WorkbookPage 1 PERIODIC TABLE OF ELEMENTS PERIOD 12131415161718 1 1HHydrogen 1.008 2He Helium 4.003 2 3LiLithium 6.941 4Be Beryllium 9.012 GROUP 5B Boron 10.811 6C Carbon 12.011 7N Nitrogen 14.007 8O Oxygen15.999 9F Fluorine 18.998 10 Ne Neon 20.180 3 11 Na Sodium 22.990 12 Mg Magnesium 24.305 3 4 5 6 7 8 9 10 11 1213 Al Aluminium 26.982 14 Si Silicon 28.086 15 P Phosphorus 30.974 16 S Sulphur 32.065 17 Cl Chlorine 35.453 18 Ar Argon 39.948 4 19K Potassium 39.098 20Ca Calcium 40.078 21 Sc Scandium 44.956 22Ti Titanium 47.867 23V Vanadium 50.942 24 Cr Chromium 51.996 25 Mn Manganese54.938 26 Fe Iron 55.845 27 Co Cobalt 58.933 28 Ni Nickel 58.693 29 Cu Copper 63.546 30 Zn Zinc 65.380 31 Ga Gallium 69.723 32 Ge Germanium 72.640 33 As Arsenic 74.922 34 Se Selenium 78.960 35 Br Bromine 79.904 36 Kr Krypton 83.798 5 37 Rb Rubidium 85.468 38Sr Strontium 87.620 39 Y Ytrium 88.906 40 Zr Zirconium 91.224 41Nb Niobium 92.906 42 Mo Molybdenum 95.940 43 Tc Technetium 98.91 44 Ru Ruthenium 101.070 45 Rh Rhodium 102.906 46 Pd Palladium 106.42 47 Ag Silver 107.870 48 Cd Cadmium 112.411 49 In Indium 114.428 50 Sn Tin 118.710 51 Sb Antimony 121.760 52 Te Tellurium 127.600 53 I Iodine 126.904 54 Xe Xenon 131.293 6 55Cs Caesium 132.905 56Ba Barium 137.327 71 Lu Lutetium 174.967 72 Hf Hafnium 178.490 73 Ta Tantalum 180.948 74 W Tungsten183.840 75 Re Rhenium 186.207 76 Os Osmium 190.230 77 Ir Iridium 192.217 78 Pt Platinum 195.064 79 Au Gold 196.967 80 Hg Mercury 200.590 81 Tl Thallium 204.383 82 Pb Lead207.200 83 Bi Bismuth208.980 84 Po Polonium (209) 85 At Astatine (210) 86 Rn Radon (222) 7 87Fr Francium (223) 88 Ra Radium 226.030 103 Lr Lawrencium 262.100 104 Rf Rutherfordium (267) 105 Db Dubnium (268) 106 Sg Seaborgium (271) 107 Bh Bohrium (272) 108Hs Hassium (269) 109 Mt Meitnerium (268) 110 Ds Darmstadium (271) 111 Rg Roentgenium (280) 112 Cn Copernicium (285) 113 Uut Ununtrium (284) 114 Fl Flerovium (289) 115 Uup Ununpentium (288) 116 Lv Livermorium (293) 117 Uus Ununseptium 118 Uuo Ununoctium (294) KEY 57 La Lanthanum133.905 Atomic Number SymbolNameRelativeatomic mass57La Lanthanum 138.905 58 Ce Cerium 140.116 59 Pr Praseodymium 140.908 60 Nd Neodymium 144.242 61 Pm Promethium (145) 62 Sm Samarium 150.360 63 Eu Europium 151.964 64 Gd Gadolinium 157.250 65 TbTerbium 158.925 66 Dy Dysprosium 162.500 67 Ho Holmium 164.930 68 Er Erbium 167.259 69 Tm Thulium 168.934 70 Yb Ytterbium 173.054 metalloids 89Ac Actinium (227) 90 Th Thorium 232.038 91 Pa Protactinium 231.036 92 U Uranium 238.029 93 Np Neptunium (237) 94 Pu Plutonium (244) 95 Am Americium (2443) 96 Cm Curium (247) 97 Bk Berkelium (247) 98 Cf Californium (251) 99 Es Einsteinium (252) 100 Fm Fermium (257) 101 Md Mendelevium (258) 102 No Nobelium (259) WorkbookPage 2 WorkbookPage 3 TUTORIAL EXERCISES This workbook is a record of your work and will assist greatly at revision time before exams. BRING THIS BOOKLET TO ALL LESSONS. Answer the following questions in the workbook during tutorial sessions. Solutions will be available on the portal (elearning.bradford.edu.au) periodically throughout the semester. It is essential that you complete all tutorial exercises either in class or as part of your homework. Seek assistance from either your teacher or access learning support sessions if needed. Textbooks See Barr Smith Library (University campus) or purchase your own. Recommendations for Adelaide University first year chemistry.Chemistry (2nd ed) by Blackman et al Introduction to Chemistry (4th ed) by Nivaldo Tro These textbooks can be purchased new from Unibooks on the Adelaide University campus or secondhand from various places (see teachers for more details on locations for secondhand textbooks) Topics this semester include: -Energy -Organic Chemistry -Rates of Reaction -Chemical Equilibrium -Acids and Bases WorkbookPage 4 ENERGY 1 1.When 4 moles of ammonia gas reacts with 7 moles of oxygen gas to form 4 moles of nitrogen dioxide gas and 6 moles of steam (gaseous water), 1132 kJ of heat energy is given out to the environment. a.Write a thermochemical equation for this reaction. b.If the activation energy for the reaction is +200 kJ, sketch the reaction profile for the reaction.Make sure you label the reactants, products, activation energy and enthalpy change. c.Draw a similar sketch for the reverse reaction, labelling the reactants, products, activation energy and enthalpy change. d.Calculate the enthalpy change when 12 moles of ammonia gas reacts with 21 moles of oxygen gas. e.Calculate the enthalpy change when 8 moles of nitrogen dioxide gas reacts with 12 moles of steam in the reverse direction. WorkbookPage 5 2.List the conditions required for measuring the standard enthalpy change of a reaction. 3.Write the chemical equations corresponding to the following standard enthalpies. a.Standard enthalpy of combustion of propanol (C3H7OH(l)). b.Standard enthalpy of formation of pentanoic acid (C4H9COOH(l)). c.Standard enthalpy of formation of sulphuric acid (H2SO4(l)). d.Standard enthalpy of neutralisation of nitric acid and barium hydroxide. e.Standard enthalpy of solution of magnesium sulphate. 4.Write the thermochemical equations corresponding to the following information. a.The standard enthalpy of combustion of butane (C4H10) is -2874 kJ/mol. b.The standard enthalpy of solution of potassium hydroxide is -55.0 kJ/mol WorkbookPage 6 ENERGY 2 1.A student poured 55.0 mL of 1.30 mol/L nitric acid into a polystyrene cup and noted that the temperature was 23.5oC.She then added 55.0 mL of 1.30 mol/L KOH and found the temperature rose to 31.8oC.Calculate the enthalpy of neutralisation, given that the specific heat of water is 4.18 J/gK and the density of the solutions was 1.00 g/mL. 2.In a laboratory experiment, 1.45 g of propanone (C3H6O) was burned completely in oxygen.This heat from this combustion was used to raise the temperature of 100g of water from 293.1K to 351.2K.Calculate the enthalpy of combustion of propanone in kJ/mol. WorkbookPage 7 3.Calculate the standard enthalpy change for the reduction of calcium chloride to calcium by sodium metal. CaCl2(s)+2Na(s)Ca(s)+2NaCl(s) Given that the following were performed under standard conditions: Ca(s)+Cl2(g)CaCl2(s)Ho = -796 kJ/mol Na(s)+Cl2(g)NaCl(s)Ho = -411 kJ/mol 4.a. Define the term standard enthalpy of formation. b. Write the equation for the standard enthalpy of formation of liquid methyl benzene (C7H8(l)).

c. State Hesss Law. WorkbookPage 8 d.Use the standard enthalpy of combustion data in the table below to calculate the standard enthalpy of formation of methyl benzene (C7H8(l)). SubstanceC(graphite)H2(g)C7H8(l) Hoc (kJ/mol)-394-286-3909 5.Propane is the fuel used in barbeque gas bottles.The complete combustion of 10.0g of propane produces 503kJ of heat. a.Write an equation for the combustion of propane b.Calculate the enthalpy of combustion of propane gas in kJ/mol. WorkbookPage 9 c.The enthalpy of combustion of propane (C3H8(g)) can also be calculated using Hesss Law.You are provided with the following information which were performed under standard conditions. 3C(s)+4H2(g)C3H8(g)H1 = -104 kJ C(s)+O2(g)CO2(g)H2 = -394 kJ H2(g)+O2(g)H2O(l)H3 = -286 kJ i.These thermochemical equations all represent a particular type of enthalpy change.What do we call this enthalpy change? ii. Use these values to calculate the Standard Enthalpy of Combustion ofpropane. WorkbookPage 10 6.In question 5 you have used enthalpy of formation data to calculate the enthalpy of combustion of propane.By a similar method you can calculate the enthalpy of formation of propane using enthalpy of combustion data.Use the combustion data below to calculate Hof for propane: C(graphite)+O2(g) CO2(g)H = -394 kJ H2(g)+ O2(g)H2O(l)H = -286 kJ C3H8(g)+5O2(g)3CO2(g) +4H2O(l) H = -2222 kJ WorkbookPage 11 7.A number of alcohols were ignited and the amount of heat given out determined.The results obtained were:

AlcoholMass of alcohol (g) Heat given out (kJ) Number of moles (mol) Methanol (3CH OH ) 3.271 Ethanol( )2 5C H OH9.2268 Propan-1-ol( )3 7C H OH7.5252 Butan-1-ol( )4 9C H OH7.4263 a.Express the energy given out by each alcohol as: i.kJ/g ii.kJ/mol b.Now write balanced thermochemical equations for each reaction. c.Comment on which is the most efficient fuel out of the four alcohols. WorkbookPage 12 8.a.Given that the enthalpy of combustion of carbon as graphite is -393.5 kJ/mol and the enthalpy of combustion of carbon as diamond is -395.4 kJ/mol, calculate the enthalpy change for the conversion of graphite to diamond. b.Which is the lowest energy form of carbon? 9.Given that the enthalpy of solution of ammonium chloride (NH4Cl) is +15.5 kJ/mol, calculate the final temperature when 2.46 g of ammonium chloride is dissolved in 100 ml of water initially at 25.1oC. WorkbookPage 13 10.Calcium oxide reacts with water as follows: CaO(s)+ H2O(l)Ca(OH)2(s) a.Given the following data calculate the enthalpy of reaction for this reaction. Ca(s) + O2(g)CaO(s) Ho = -636 kJ/mol 2H2(g) + O2(g) 2H2O(l)Ho = -572 kJ/mol Ca(s) + O2(g) + H2(g) Ca(OH)2(s)Ho = -987 kJ/mol b.How much water, initially at 20oC could be boiled by the heat released when1.00 kg of calcium oxide is reacted with water, assuming there is no loss of heat? WorkbookPage 14 ENERGY 3 1.The reaction between aqueous sodium hydroxide and hydrochloric acid solution has a H value of -57 KJ mol-1. a.Write a thermochemical equation for this reaction. b.What type of reaction has occurred? c.Will the temperature of the solution increase or decrease when the two substances react? Explain. d.Draw an energy profile diagram for the reaction. 2.The enthalpy of combustion value of liquid cyclohexane (C6H12) is 3916 KJ mol-1. a.Write a thermochemical equation for this reaction. b.Calculate how much heat will be produced when 1.00g of liquid cyclohexane undergoes complete combustion. 3.Write thermochemical equations for the following: a.The standard enthalpy of combustion of butane gas is -2874 kJ/mol. b.4 moles of butane gas are burnt. c. 12 moles of butane gas are burnt. d.The standard enthalpy of formation of water is -286 kJ/mol. WorkbookPage 15 4.In an experiment to determine the standard enthalpy of solution of potassium hydroxide, 4.09g of potassium hydroxide was added to 100mL of water, at 18.5 oC, in a polystyrene cup. The solution was stirred until all the solid had dissolved and the maximum temperature reached was 28.1 oC. Assume the specific heat capacity of the solution is 4.18 Jg-1oC-1.a. Calculate the standard enthalpy of the solution. b.Calculate the temperature change which would occur if 2.53g of potassium hydroxide was dissolved in 150 mL of water. c.Calculate the mass of potassium hydroxide which would have to be dissolved in 200 mL of water to bring about a 10 oC rise in temperature of the water. 5.Given the following data: kJ H g NO g O g Nmol kJ H g NH g N g Hmol kJ H g NO g O g Nmol kJ H g O H g O g H34 ) ( ) ( ) (21/ 46 ) ( ) (21) (23/ 90 ) ( ) (21) (21/ 242 ) ( ) (21) (2 2 23 2 22 22 2 2+ = A + = A ++ = A + = A + Calculate the H values for the following reactions: a.) ( 4 ) ( 6 ) ( 5 ) ( 42 2 3g NO g O H g O g NH + + b.) ( 2 ) ( ) ( 22 2g NO g O g NO + WorkbookPage 16 ORGANIC 1 1.a.Carbon shows tetravalence in its compounds. Explain this term. b.Describe the shape of the four single covalent bonds around a carbon atom in carbon compounds. c.What is the angle between two single bonds in carbon compounds, ie the H -C - H bond? d.The length of the carbon to carbon bond is 1.54 A. (A is the angstrom unit which is used to measure bond length).Explain why the distance between the first and last carbon atoms in propane is 2.54A and not 3.08A. 2.Write the molecular formula and give the names for the following molecules: a. A molecule with eight carbon atoms and the general formula CnH2n b. A molecule with five carbon atoms and the general formula CnH2n-2 c.A molecule with six carbon atoms and 14 hydrogen atoms WorkbookPage 17 3.a.Explain the difference between the molecular formula and structural formula. b.Write the structural formula(s) of butene. c.Write the molecular formulae of butene. 4.Consider the sixth member of the alkane homologous series.If the molecule is unbranched (no side chains) give: a.Its name. b.Its molecular formula. c.Its empirical formula. d.Draw out its structural formula. e.Write the structural formula in condensed form. WorkbookPage 18 f.Now by considering possible side chains draw and name as many structural isomers as you can for this molecule (remember the isomers must all have the same molecular formula). 5.a.Explain the term homologous series giving some of the properties of a series. b.The alkanes are a saturated homologous series. The alkenes are an unsaturated homologous series. Explain the terms saturated and unsaturated giving a hydrocarbon example of each. WorkbookPage 19 c.Which of the following molecules are saturated? i)2-methylpentane ii)1-Butene iii)3-methyl-1-pentyne Which is the most unsaturated? d.Name the functional group in the alkenes. 6a.Write the equation for the reaction between ethane and chlorine gas in the presence of sunlight (UV light).What type of reaction is this? b. Write the equation for the reaction between ethene and bromine gas. What type of reaction is this? c. Write the equation for the reaction between propene and HCl.What type of reaction is this?Is there more than one possible product? WorkbookPage 20 7.How many products are obtained from: a.A substitution reaction b.An addition reaction c.What product(s) are obtained when propene and hydrogen gas are mixed at room temperature 8.a.Write the equation for the complete combustion of octane b.What would the combustion products be if the combustion was incomplete (i.e. occurred in limited oxygen)? c.Why is a bunsen burner flame yellow when the air hole is closed? WorkbookPage 21 9.Butanone, pentanone and hexanone are all members of the ketone homologous series. a.What can we say about their chemical properties? b.What can we say about their physical properties (e.g. melting point)? c.If the molecular formula of butanone is C4H8O, what is the general formula of the ketones? d.What is the molecular formula of hexanone? WorkbookPage 22 ORGANIC 2 1.Give the systematic names for the following: a. CH3CH=CHCH3b. CH3CH=CHCH2Br

c. CH3CH2CHCH2CH2OHd. CH2FCH2CHBrCH=CFCH3 2.Draw structural formulae for the following: a. 2-methylpentaneb. trichloromethane c. 3-methyl-2-pentanold.1,2,4,4-tetrabromo-1-hexene e.8-bromo-1-iodo-1-octanolf. 2-methylbutanoic acid CH3 WorkbookPage 23 3.Give the structural formula and names for the product(s) of the following reactions (assume the appropriate conditions and catalysts are present): a.Propane gas and chlorine gas. b.Propene gas and bromine liquid. c.Butene gas and steam. d.Pentene and hydrogen. e.1-hexene liquid and hydrochloric acid. WorkbookPage 24 4.Give the name and structure for all compounds with the following formulae: a.C4H10 b.C6H14 c. C5H10 WorkbookPage 25 5.Define the term structural isomer. 6."PhiltheDill"drewstructuralformulaefortwoorganiccompoundsthathenamed3-methyl butane and 1,2 dimethylethene. "Wayne the Wally" said that the compounds may well exist but said his naming of them was wrong. Draw the structures and rename them correctly. 7.Name the organic molecules shown below: a. HC H H C H H C H H C O OH ------------------------------------------------------------------------------

b. HC HHCHCH3OH --------------------------------------------------------------------------------- c. H CHHCCH3HCHHCOO H ----------------------------------------------------------------------------- d. H 3 CC F CH 3 C H CH 3 C H H CH 3 -------------------------------------------------------------------------------- WorkbookPage 26 ORGANIC 3 1.For each of the following alcohols i.Draw the structural formula ii.Name the alcohol iii.Classify as either primary, secondary or tertiary. a. 3 2 3) ( CH OH CH CH CH b.COH CH3 3) ( c.CHOH CH2 3) ( d.OH CH CH CH2 4 2 3) ( 2.For the following draw structural diagrams and classify as primary, secondary or tertiary.a.2 propanol b.3 methyl 2 butanol c.2 methyl- 1 pentanol WorkbookPage 27 d.Ethanol e.3 ethyl 3 hexanol f.1, 2 - ethandiol 3.1 propanol is mixed with acidified potassium dichromate solution. a.What colour change will be observed? b.Draw the structural diagrams of the products that will be produced. c.Write half equations for the production of each of the products formed. d.Write an overall equation for the oxidation of 1 propanol. e.If 2 propanol was used instead, are the same products formed? If not draw the new product/s. WorkbookPage 28 4.Explain why ethanol is soluble in water whereas octanol is not soluble. 5.Although they have similar molecular masses, there is a significant difference in the boiling points of butane, 0oC, and 1- propanol, 97oC. Draw the structures of both compounds to help explain the difference in boiling points. 6.Alcohols can be prepared a number of ways. Write balance equations, include any conditions required, and name the type of reaction that has occurred (i.e. addition, substitution or fermentation) for the production of the following: a. 2 butanol from butene b.Ethanol from glucose(6 12 6O H C ). c.1 propanol from 1- bromopropane. 7.Describe the fermentation process of making alcohol. Why are some alcohols distilled after they have undergone fermentation? WorkbookPage 29 ORGANIC 4 1.a.Draw the structural formulae of propanal2- pentanone acetone (propanone)2-chlorobutanal b.The general formula of an aldehyde is often written as RCHO.Explain the meaning of the R. c.Draw the structural formula for the first member of thealdehyde series. Write the systematic name and common name for this compound. Systematic _______________Common _________________ d.Name and draw the structural formulae for the second member ofthe ketone series. WorkbookPage 30 2.Consider the following compounds: a.CH3CH2COOHb.CH3CHO c.CH3COC2H5d.CH3OH e.CH3CH2OHf.HOOCH i.Which of these compounds would react in a similar manner to compound a. ii.Which of the compounds are in the alcohol homologous series? iii.Which of the compounds contain a carbonyl functional group? iv.Which of the compounds is a ketone? v. Which of the compounds are aldehydes? vi.Which of the compounds are carboxylic acids? 3.a.Classify the following alcohols as primary, secondary or tertiary. i.1-Butanol ii.3-methyl-2-butanol iii.2,3-dimethyl-2-pentanol b.For each of the alcohols above draw the structural formula, and name, all of the organic products formed when the compound is heated with acidified potassium dichromate. WorkbookPage 31 c.Describe how you could distinguish between the following three compounds using just two tests: 3-methyl-2-butanol,3-methylbutanal and butanone 4.The table below shows the relative molar mass of 4 compounds and their boiling points. Use these figures to answer the questions below: CompoundRelative molar massBoiling point Tb/oC Butane58-0.5 propanal5849 propanone5856 1-propanol6097 a.Is the carbonyl functional group a polar group? If so, draw itsstructure showing its polarity. b.Would there be any secondary bonding between propanal molecules? If so, is it hydrogen bonding? c.Explain why propanal has a higher boiling point than butane but lower than propan-1-ol. d.Draw a diagram showing the hydrogen bonding between a moleculeof propanal and water. Show the polarity of the bonds involved. WorkbookPage 32 e.Give the reason why propanal is soluble in water but hexanal is only slightly soluble. 5.a.Consider each of the structures below. Circle the functional groupin each structure. Write the name of each functional group. C OCH3 CH3CH2CH2CCHCH3C CH3CHCHO CH3OCHCH3H3C

acetophenonecitralmenthone CH=CHCHO cinnamaldehyde b.Each of the above substances are mixed with acidified potassiumdichromate. i.Which of the above substances would react? ii.What changes would be observed? iii.Draw structures of the organic products formed during these reactions. c.How could you identify unlabelled samples of citral and menthone?(Without using acidified potassium dichromate) WorkbookPage 33 6.a.In the preparation of butanal from 1-butanolthe acidified dichromatesolution has to be added slowly, but in the preparation of butanone from2-butanol this is not so. Explain why. b.3-methyl-2-pentanone is prepared from an alcohol. Draw the structural formula of the alcohol. Name the alcohol. c.Propanal will react with ammoniacal silver nitrate to form the carboxylateion of the corresponding acid. i.What would be observed? ii.Write an equation to explain the observation. iii.Draw the structuralformula of the carboxylate ion and name it. WorkbookPage 34 ORGANIC 5 1)a.Following is the structure of a synthetic flavour compound. i.Draw the structures of the carboxylic acid and the alcohol from which this could be prepared. Carboxylic acidAlcohol ii.Write an equation for the esterification reaction. b.Following is the structure of an ester. i.Draw the structures of the products formed when the ester undergoes hydrolysis is the presence of an acid. ii.Draw the structures of the products formed when the ester undergoes hydrolysis in the presence of a base. iii.Write an equation for the alkaline hydrolysis reaction. WorkbookPage 35 2.The ester pentyl ethanoate is found in bananas. It can be manufactured by reacting a carboxylic acid and an alcohol. i.Name and draw the structural formula of the alcohol used. ii.Name and draw the structural formula of the carboxylic acid used. iii.What other substance must be added to the preparation mixture and why is it added? iv.Draw the structure of the ester formed. v.The mixture produced is an equilibrium mixture. Explain the meaning of the term equilibrium mixture. 4.a.i.Write the molecular formulae of glucose and fructose.They are examples of which type of carbohydrate? ii.What is the name of the particular molecule formed when a glucose molecule and a fructose molecule link together? iii.What is the other product of this reaction? WorkbookPage 36 iv.What type of reaction is the formation of this new molecule v.What is the molecular formula of this new molecule? vi.What is the general name given to carbohydrates of this type? b.i.What type of carbohydrate would I have if I now linked 1000 glucose molecules? ii.What would the molecular formula of this molecule be? 5.Lactose is a major constituent of milk. The enzyme lactase hydrolyses lactose into monosaccharide products, as shown in the diagram below: a.What type of sugar is lactose? b.Write the molecular formula of lactose and give an explanation of how it conforms to the general formula of a carbohydrate. WorkbookPage 37 c.State the number of moles of monosaccharide products formed per mole of lactose hydrolysed. d.Some monosaccharides react with Tollens reagent. State what you would expect to observe that would indicate that a reaction had taken place. e.Name the functional group indicated by a positive Tollens test. WorkbookPage 38 6.Starch is a carbohydrate found in many grains. a.i.Is starch a monosaccharide; disaccharide or polysaccharide ?

ii.Explain why starch is insoluble in water while glucose is very soluble in water even though they are both carbohydrates. b.Starch can be converted into glucose. i.Write an equation for the conversion of starch into glucose. ii.What is the name given to this type of reaction ? c.Starch can be converted into lactic acid. The structure of lactic acid is shown below: HO CH C - OH i.Explain why lactic acid is not classified as a carbohydrate. ii.Explain why lactic acid is soluble in water. O CH3 WorkbookPage 39 ORGANIC 6 1.Draw structural formulae for

a.2-methyl-2-propanamine b.3-hexanamine c.N-methyl-1-propanamine d.N,N-dimethyl-1-propanamine ` e.N-ethyl-2-methyl-2-butanamine 2.Identify the compounds in question 1 as primary, secondary or tertiary amines. 3.a.Draw the structural formula of the molecules that result when 2-methyl-1-propanamine reacts with butanoic acid. a.What type of reaction is this? 4.Draw the structural formula for a 3 unit section of the polymer formed when1-butene is used as the monomer. Indicate the repeating unit. WorkbookPage 40 5.When 1,3 propandiol reacts withthe di-carboxylic acid of butane ( 1,4 dibutanoic acid ) a polymer is formed. Write down the structural formula of3 repeating units of this polymer. Place square brackets around one of the repeating units. What type of polymerisation is this reaction?

WorkbookPage 41 ORGANIC 7 1.Draw structural formulae for the following compounds a.Propanal b.2-pentanone c.methyl propanoate d.butanoic acid e.3-methyl-2-butanol f.3-methylbutanal 2.Which pairs of compounds in question 1 are structural isomers?

3.Describe the expected observation and give the name and structural formulae for any organic products formed when a, b, e and f are mixed with a. a solution of acidified potassium dichromate. a b e f b.Tollens reagent a b e f WorkbookPage 42 4.Name and give the structural formula for the organic products formed whena.c is boiled under reflux with sodium hydroxide solution. b.d and e are boiled under reflux with sulphuric acid. 5.Describe how you would go about producing a pure sample of a, b d and e in the laboratory. Include equations. a b d e 6.Describe how you would separate a mixture of a.hexananoic acid and hexane b.ethanal and ethanol WorkbookPage 43 ORGANIC 8 1.Consider the following fatty acids: A:CH3(CH2)15COOH B:CH3(CH2)7CH=CH(CH2)7COOH C:CH3(CH2)3CH=CH(CH2)3CH=CH(CH2)2CH=CHCH2COOH a.Which fatty acid is: i.saturated ii.monounsaturated iii.polyunsaturated b.Which fatty acid is most likely to derive from: i.a vegetable source ii.an animal source c.Which fatty acid is most likely to be a liquid oil at room temperature. d.Name the reagent and conditions (including catalyst) that I would use to convert this liquid oil into a solid fat. e.Draw the structure of the triglyceride that would yield all three of these fatty acids upon hydrolysis.

WorkbookPage 44 f.Name and draw the other product that would be produced by hydrolysis of this triglyceride. 2.a.Write an equation showing how a triglyceride may be formed from glycerol and stearic acid (CH3(CH2)15COOH). b.Write an equation showing alkaline hydrolysis of this triglyceride. c.Name and describe the process by which the products of this reaction are converted into soap. WorkbookPage 45 ORGANIC 9 1.a.Name and describe the process by which the triglyceride made from stearic acid (CH3(CH2)15COOH)is converted into soap. d.The soap produced by this process is sodium stearate.Draw a molecule of sodium stearate showing the hydrophobic (non-polar) end and the hydrophilic (polar end). e.Soaps tend to form micelles in water.Draw a micelle and explain how they remove grease from fabrics or skin. WorkbookPage 46 f.Explain why soaps are less effective in acidic conditions. g.Other materials are added to commercially produced soaps. One of these materials is tripolyphosphate.Give three reasons for adding this substance. 3.Sodium and potassium salts of fatty acids are soluble in water. However the Calcium and Magnesium salts are not. Write an equation to show how dissolved Calcium ions will interact with a sodium soap. WorkbookPage 47 4.A household washing powder includes sodium dodecylbenzene sulphonate CH3(CH2)11 -- SO3- Na+ Sodium dodecylbenzene sulphonate is known as an anionic surfactant. On the structural formula above, identify the hydrophobic and hydrophilic parts of the structure. a.How does a soap differ from a detergent? b.Detergents perform functions similar to those of soap. Describe the structural similarities of soap and detergent that allow them to act in the same way. c.Describe a situation in which detergents are better cleaning agents than soaps. Explain why this is so. WorkbookPage 48 RATE OF REACTION 1 1.0.21 g of powdered magnesium carbonate was added to excess hydrochloric acid and the resulting gas was collected and the volume monitored as time progressed. The result is shown in the table below. a. What is the gas produced ? b. Write a balanced chemical equation for the reaction. c. Accurately produce a labelled graph of volume of gas vs time. d.From your graph estimate the initial rate of the reaction (t=0) and the rate att = 3.0 mins in mL/min. Time (min)00.511.522.533.54567 Vol of gas (mL)01832445361677275777777 WorkbookPage 49 e.Why are the two rates different? f.Estimate the average rate over the first 3.0 minutes. g.From your graph determine the point in time (after the start) at which equilibrium was reached. 2, By reference to collision theory, explain the effect on reaction rate of increasing each of the following quantities: a.Concentration (in a solution) b.Pressure (of a gas) WorkbookPage 50 c.Surface area (of a solid) d.Temperature (of a gas or solution) 3.Draw the reaction profile for an endothermic reaction both with and without a catalyst.In each case label the enthalpy change and the Activation Energy. 4.List 3 mechanisms by which a catalyst can increase the rate of a reaction. WorkbookPage 51 5.a.Sketch Maxwell-Boltzmann Distributions for a gas mixture at 25C and 100C.By reference to areas under the curve, explain why reaction rate will be higher at 100C than 25C. b.On a separate axis sketch a Maxwell-Boltzmann Distribution for a gas mixture at 25C.By reference to areas under the curve, explain how adding a catalyst increases the rate of reaction. WorkbookPage 52 RATE OF REACTION 2 1.What is the effect of adding a catalyst on: a.The reaction rate. b.The Activation Energy (EA) c.The Enthalpy Change (H) 2.The reaction A + B + C C + D was found to be second order with respectto A, first order with respect to B and zero order with respect to C. a.Write the Rate Law for the reaction. b.What is the effect on the rate of increasing the concentration of A by a factor of 4? c.What is the effect on the rate of halving the concentration of B? d.What is the effect on the rate of doubling the concentration of C? e.What is the effect on the rate constant of doubling the concentration of A? f.What is the effect on the rate constant of increasing the temperature by 20C? WorkbookPage 53 3.The following initial rate data were obtained at 60C for the reaction: A + B C [A] (molL-1)[B] (molL-1)Rate (molL-1s-1) 0.250.250.0147 0.500.250.0294 0.500.500.0588 a.Determine the Rate Law for the reaction at 60C (including the value of k). b.Hence determine the initial rate at 60C when the initial concentration of A is 0.80 molL-1 and the initial concentration of B is 0.60 molL-1. WorkbookPage 54 EQUILIBRIUM 1 1.a.In the production of sulphuric acid sulphur trioxide gas is converted tosulphur trioxide gas by the addition of oxygen. 2SO2(g) + O2(g) 2SO3(g) Write an equilibrium expression for this reaction. A reaction vessel of 10 L has 2.0 moles of sulphur trioxide present atequilibrium and 0.37 moles of each of the other gases. Calculate the value of Kc. In another container the same reaction takes place. Find the concentration of sulphur trioxide if the concentration of sulphur dioxide and oxygen areboth 0.10 molL-1. WorkbookPage 55 2.Ammonia is manufactured by combining the two gases ammonia andhydrogen. The equation is N2(g) + 3H2(g)2NH3(g) The reaction vessel of 0.40 L originally contained 2.0 moles of nitrogen gas and 6.0 moles of hydrogen gas. At equilibrium it was found 2 moles of ammonia were present. a.Calculate the equilibrium constant at that temperature. b.If this reaction takes 5 minutes to come to equilibrium, sketch (on the same graph) the concentration vs. Time curve for each reactant and product. WorkbookPage 56 3.Dinitrogen tetroxide will form an equilibrium with nitrogen dioxide in a closed vessel. N2O42NO2 At 100oC the equilibrium constant for this reaction is 45. Calculate the concentration of nitrogen dioxide gas if at equilibrium the moles of dinitrogen tetroxide is 0.050 in a 10L vessel. 4.Carbon dioxide and hydrogen will react at high temperatures to form the poisonous carbon monoxide and water vapour. The equation is CO2 +H2 CO+H2O a.Write an expression for the equilibrium constant. b.Carbon dioxide and hydrogen were placed in a reaction vessel and equilibrium was attained at 600oC. 0.40 mole of carbon dioxide and 0.40mole of hydrogen were initially placed in a 2.0L reaction vessel. Atequilibrium there was 0.30 mole of water vapour. Calculate: i.the moles of each substance at equilibrium WorkbookPage 57 ii.the equilibrium concentrations of each substance iii.the value of Kc 5.When 0.7 moles of phosphorus pentachloride is maintained at 250 oC in a2 litre vessel, equilibrium is attained when 0.2 mole phosphorus trichloride has formed. Write down the concentration of each species present at equilibrium, and find the equilibrium constant, Kc for the reaction: WorkbookPage 58 EQUILIBRIUM 2 1. Indicate which way each of the following reactions at equilibrium will shift when the concentration of one of its components is changed as indicated: a. H2(g) + I2(g)2HI(g) (concentration of iodine is increased) b. N2(g) + 3H2(g)2NH3(g) (ammonia is removed from the system) c. 2NO2(g)2NO(g) + O2(g) (reaction occurs in pure oxygen instead of air). 2. Determine how each of the following reactions at equilibrium would be changed by an increase in pressure: a. H2(g) + Br2(g) 2HBr(g) b. CH4(g) + 4CuO(s)CO2(g) + 2H2O(g) + 4Cu(s) c. C2H4(g) + 3O2(g)2CO2(g) + 2H2O(l) 3. Determine whether an increase or decrease in temperature will increase the value of the equilibrium constant in each of the following equilibrium systems: a. C(s) + O2(g)CO2(g) (93.4 kJ released per mole of CO2 formed) b. H2(g) + I2(g) 2HI(g) (5.93 kJ absorbed per mole HI formed) c. CH4(g) + 4CuO(s)CO2(g) + 2H2O(l) + 4Cu(s) (15.6 kJ released per mole of Cu formed) 4. The system: N2(g) + O2(g) 2NO(g) is at equilibrium. The formation of each mole of nitrogen (II) oxide consumes approximately 22 kJ. How will the equilibrium constant be affected in each of the following cases? a. The temperature is increased by 25 oC. b.The pressure is cut in half. c. The source of nitrogen becomes contaminated with a 20% mixture of helium. d.The nitrogen (II) oxide is drawn off at the rate of 0.54 grams per minute. WorkbookPage 59 5.Methanol is produced by the reaction CO(g) +2H2(g) CH3OH(g) a.Write an expression for the value of Kc. b.In your own words, explain Le Chatelier's Principle. c.The above equilibrium was established in a closed vessel. The volume of the vessel was quickly reduced to half. What affect does this have on the amount of methanol in the equilibrium mixture? Explain. d.What effect will this have on the value of Kc? e.The equation as written is exothermic. What will happen to theamount of methanol in the equilibrium mixture if the temperature is increased? Explain. f.What effect will this have on the value of Kc? WorkbookPage 60 7. A mole of hydrogen and a mole of iodine are put in a 10 litre container at520 oC and allowed to come to equilibrium. Analysis of the equilibrium system shows that 0.12 moles of hydrogen iodide is present. Find the equilibrium constant, Kc, for the reaction at 520 oC. 8. Consider the equilibrium reaction: PCl5(g) PCl3(g) + Cl2(g) at 250 oC a. Suppose 1.00 mole of phosphorus pentachloride was introduced into the reaction vessel at the start of the reaction. if at the end of the reaction, there was only 0.75 moles left, how much of the following was produced (i) chlorine, (ii) phosphorus trichloride? (b) If 1.00 mole of phosphorus pentachloride had been introduced and x moles now remain, how many moles of phosphorus trichloride would be present? (c) A 1.00 mole sample of phosphorus pentachloride was put into a ten litre container. Later the amount of phosphorus pentachloride which remained was 0.30 mole. What was the concentration of phosphorus trichloride? WorkbookPage 61 9. The formation of the ester called ethyl acetate by reaction between acetic acid and ethanol is an equilibrium reaction represented by the equation: CH3COOH(l) + C2H5OH(l) CH3COOC2H5(l) + H2O(l) Ethyl acetate is usually made from glacial acetic acid and pure ethanol. All of the substances present at equilibrium are liquids. a.Write the equilibrium expression for this reaction. Note in this reaction water is NOT a solvent present in large excess. b.When 1.00 mole of acetic acid is mixed with 0.18 mole of ethanol, there is 0.171 mole of ethyl acetate in the final equilibrium mixture at 20 oC. Calculate the amounts, in moles, at equilibrium of (i) acetic acid, (ii) ethanol, (iii) water. c.From the equilibrium amounts, calculate Kc at 20 oC. d.1.000 mole of acetic acid is mixed with 8.000 mole of ethanol and the temperature maintained at 20 oC. After some time, the amount of ethyl acetate present was measured to be 0.966 moles. Is this reaction at equilibrium yet? e.1.000 mole of acetic acid is mixed with with 8.000 mole of ethanol and the temperature kept at 20 oC. After some time, the amount of ethyl acetate was 0.214 mole. Is this reaction at equilibrium yet? WorkbookPage 62 EQUILIBRIUM 3 1.Dinitrogen trioxide decomposes according to the following equation. 1) ( 2 ) ( ) ( 3 25 . 40+ = A + KJmol H NO NO O Ng g g Predict the effect of the following changes on the position of the equilibrium (left, right or no change) and the value of Kc when each of the following changes is made. a.Adding more N2O3(g) b.Adding more NO2(g) c.Increasing the volume of the reaction flask d.Lowering the temperature. e.The reaction flask was not sealed 2.At a particular temperature some sulphur dioxide gas and some nitrogen dioxide gas were placed into an empty flask which was sealed. After t1 seconds, the following equilibrium was established. ) ( 3 ) ( ) ( 2 ) ( 2 g g g gSO NO SO NO + +a.Sketch a graph, on the set of axes below, of the forward and back reactions against time from the start to sometime t2 after equilibrium was established. b.On the same axes, sketch a graph if a catalyst was used at the start of the reaction. Time (sec) Rate of reaction (Ls-1) WorkbookPage 63 3. For the following reaction:KJ H g Br g NO g NOBr 1 . 16 ) ( ) ( 2 ) ( 22+ = A + , predict the effect of the following changes on the position of equilibrium (state if it will shift left, right or no change). a.Adding more Br2(g) b.Removing some NOBr(g) c.Decreasing the temperature d.Increasing the container volume 4.Methanol can be produced industrially using the following two processes: Reaction 1 : 1) ( 2 ) ( ) ( 2 ) ( 4208 3+ = A + + KJmol H H CO O H CHg gNig g Reaction 2 : ) ( 3 ) ( 2 ) (2gZnOg gOH CH H CO +1103 = A KJmol H a.State two conditions needed for the chemical systems to establish equilibrium. b.Predict the conditions of temperature and pressure (high/low) which will maximise the yields of the products of reaction 1 and 2. ReactionPredicted temperature (high/low)Predicted pressure (high low) 1 2 Reasons for your predictions: Temperature: Pressure: c.For reaction 1, explain the role of nickel. WorkbookPage 64 d.Draw energy profile diagrams for both reactions. Label reactants, products, enthalpy and activation energy. e.For all exothermic reactions in industry, there is a compromise between yield and rate when selecting an operating temperature. Explain the meaning of this statement with reference to reaction 2.

5.The graph below represents the production of ammonia which was carried out in a closed reaction flask. a.Write the equilibrium expression Kc for the reaction and calculate its value using the concentrations during the first 10 mins. b.Suggest the change that occurred at 10 minutes and explain the changes that occurred in the flask in the following 2 minutes. c.At what time was equilibrium re-established? How can you recognise this? WorkbookPage 65 d.Calculate the value of Kc using the concentrations at the 20 minute mark. e.At 25 minutes, more nitrogen was added to the flask. Extend the graph to show the effect of the addition of the gas. 6.Kc for the decomposition of ammonium hydrogen sulphide is 410 8 . 1at 25oC. ) ( 2 ) ( 3 ) ( 4 g g sS H NH HS NH + a.Write the equilibrium expression for the decomposition of ammonium hydrogen sulphide. b.When the pure salt decomposes in a flask, what are the equilibrium concentrations of NH3 and H2S? c.If NH4HS is placed in a flask which way will the equilibrium shift? d.If NH4HS is placed in a flask already containing 0.020 molL-1 of NH3 and the system is allowed to equilibrium, what are the equilibrium concentrations of NH3 and H2S? WorkbookPage 66 ACIDS & BASES 1 1.Write the equation for the ionisation of nitric acid. 2.Write the equations for each of the ionisation reactions of phosphoric acid. 3.Write balanced equations for the following reactions. a.Sulphuric acid and magnesium b.Nitric acid and potassium hydroxide c.Ethanoic acid and sodium hydrogen carbonate WorkbookPage 67 4.Write balanced equations (or indicate no reaction) for the reaction of hydrochloric acid and sodium hydroxide with each of the following. asodium oxide baluminium oxide csulphur dioxide 5.Given that a hydrogen ion is simply a proton, what must a base have to accept a proton? 6.Write expressions for the following aThe ionic product (Kw) of water. bThe solubility product (Ksp) of potassium chloride. cThe ionization constant (Ka) of nitric acid. WorkbookPage 68 d.How do you convert Ka to pKa? e.How do you convert pKw to Kw? 7.Make the following conversions: i.Calculate pKw if Kw = 1x10-14 ii.Calculate Ka if pKa = 5.32 iii.CalculatepKa if Ka = 3.4x10-13 8.Which of the following reactions are acid-base (protolysis) reactions: i.NH3(g)+HCl(g)NH4+ +Cl- i.2H2O2(l) H2O(l)+O2(g) ii.HSO4-(aq)+OH-(aq) SO42-(aq)+H2O(l) WorkbookPage 69 9.Calculate the pH and pOH of the following strong acid and strong base solutions at 25oC. i.1x10-3M HCl ii.10.0M HCl iii.1x10-5M NaOH iv.5.0M Ba(OH)2 v.6.37x10-4M HNO3 vi.0.0023M KOH 10. Calculate the hydronium and hydroxide ion concentration in the following solutions at 25oC: i.a solution of pH = 3 ii.a solution of pH 9.34 WorkbookPage 70 iii.a solution of pOH = 9.34 11. If I mix 50.0 ml of 0.050 M HCl with 30 ml of 0.020 M Ba(OH)2, what is the pH of the resulting solution at 25oC. 12. If the Kw of water at 100oC is 1x10-13, what is the pH ofpure water at 100oC? WorkbookPage 71 ACIDS & BASES 2 1.Write balanced equations for the following reactions and identify the acid / base conjugate pairs. a.Sulphuric acid and lithium hydroxide b.Nitric acid and potassium hydroxide c.Acetic(ethanoic) acid and sodium hydrogen carbonate 2.Define the term amphoteric and give an example of an amphoteric substance including equations illustrating its amphoteric nature. 3.Define the term amphiprotic and give an example of an amphiprotic substance including equations illustrating its amphiprotic nature. WorkbookPage 72 4.a.Estimate what you think the pH of a solution of acetate (ethanoate) ions would be, and explain the reasons for your answer. (write an equation) b. Estimate what you think the pH of a solution of ammonium chloride would be, and explain the reasons for your answer. (write an equation ) 5.a.Calculate the pH of a 0.25 M solution of ethanoic acid (Ka = 1.8x10-5). b.Lactic acid is a carboxylic acid with the formula CH3CHOHCOOH. Calculate the pH of a 0.005M solution of lactic acid (pKa = 3.07) WorkbookPage 73 6.Lactic acid is a carboxylic acid with the formula CH3CHOHCOOH. Explain, with the aid of an equation, how a solution of0.1M lactic acid and 0.1M Sodium lactate maintains an almost constant pH when small amounts of acid or base are added to it. 7. Calculate the pH of the following solutions i.0.05 MHCl ii.0.04 M NaOH iii.1.2 M Ba(OH)2 iv.0.2 M CH3COOH, Ka = 1.8x 10-5 v.0.002 M HA, pKa = 3.7 WorkbookPage 74 8.Identify the conjugate of each of the following species. NH2- CN- NH4+

HCO3-

H2SO4

H2PO4- OH-

NO2- 9.Write two equations for reactions that illustrate the amphiprotic nature of the hydrogen carbonate ion. 10. Would the following solutions be acidic, basic or neutral. Explain using an equation where necessary i.Sodium chloride. ii.Ammonium Nitrate WorkbookPage 75 iii.Potassium Ethanoate iv.Sodium Hydrogen Carbonate v.Potassium Nitrate WorkbookPage 76 GROUP WORK ACTIVITES The following activities are to be completed in class in group situations. They will help with understanding the topic material and your ability to work and communicate with different people. They are designed to improve your thinking and discussion skills. Activity 1 Energy Enthalpy is the amount of heat energy absorbed or released during a reaction under constant pressure. Lists of standard enthalpy values for formation reactions are usually included in the appendix of textbooks. For example Substance) (1 A mol KJ H fo ) ( 5 2 lOH H C-277.63 ) ( gHCN+135.1 ) ( 4 sCuSO-771.4 ) ( 2 lO H-241.8 ) (sNaCl-411.0 Scientists measure the energy absorbed or released in a reaction by using a bomb calorimeter. To use a bomb calorimeter the substance to be tested is burned in a metal chamber that is well insulated with water. Heat formed by burning is transferred to the water and the temperature is measured. Both the mass of the water and the substance are recorded. In a school laboratory a simple calorimeter is made using styrofoam cups (refer to practical 7). When using the simple calorimeter method, the experimental value calculated is different to the theoretical values that are found in textbooks. Discuss and record at least five reasons as to why these values differ? WorkbookPage 77 Activity 2 Organic Chemistry Organic chemistry is the study of carbon compounds. It is also known as the chemistry of life. We have studied the following organic compounds: hydrocarbons, alcohols, aldehydes, ketones, carboxylic acids, amines and esters. In particular we have learnt how to name the different compounds. 1.Write the systematic name for the following compounds and circle the functional group. 2.Explain why the following compounds are named incorrectly. Write the correct name. ethyl pentanoate3, 5-dimethyl hexane WorkbookPage 78 3.There are many ways to draw the structural formula of an organic compound. For example: 2-methyl pentane can be drawn the following ways. Using the structures above, draw the different types of structural formula for the following compounds: a.2, 3-dimethyl hexane b.1-chloro-2-butene c.3-ethyl-4-heptanol 4.Draw three challenging organic structures that are nameable using the rules we have learnt. These structures will be collected and collated for a competitive group vs group quiz. WorkbookPage 79 Activity 3 Rates of reaction We have discussed how rate depends on the concentration of reactants by looking at the rates laws. For the equation ( ) ( ) ( ) g g gA B C +| | ARatetA=A First order rate law:| |Rate k A =Second order rate law: | |2Rate k A =Zero order rate law:Rate k = A more useful rate law can describe how the concentration changes over time. Using calculus, we can use integration to find the integrated rate laws. 1.Show the integrated first order rate law is described by: | | | |0ln ln A kt A = + . (Note [A]0 is the initial concentration of A.) Extension: 2.Show the integrated second order rate law is described by:| | | |01 1ktA A= + 3.Show the integrated zero order rate law is described by:| | | |0A kt A = + WorkbookPage 80 ( ) ( ) 2( )2 2g g gNOCl NO Cl +Activity 4 Equilibrium The equilibrium constant is based on experiments. It tells us when an experiment has reached equilibrium. Compete the following involving the equilibrium constant. 1.Calculate the value of K. A 3.0 L flask initially contains 2.4 mol of Cl2, 1.0 mol NOCl, and 4.5 mol of NO at a constant temperature. Calculate the equilibrium constant if there contains 1.5 mol of NOCl at equilibrium. The equation for the reaction is 2.Calculate the equilibrium concentration. Carbon monoxide reacts with stem to produce carbon dioxide and hydrogen. At 700 K the equilibrium constant is 5.10. Calculate the equilibrium concentrations of all species if 1.00 moles of each component is mixed in a 1.00 L flask. WorkbookPage 81 2( ) 2( ) 3( )2 2g g gSO O SO +3.Calculate the equilibrium concentration. The reaction for the formation of gaseous hydrogen fluoride from hydrogen and fluorine has an equilibrium constant of 1.15 102 at a certain temperature. If 3.00 mol of each component was added to a 1.50 L flask, calculate the equilibrium concentrations of all species. 4.Effect on K if a change in concentration occurs. The following results were collected for the following reaction performed at a constant temperature, Experiment 1Experiment 2 Initial (mol L-1)Final (mol L-1)Initial (mol L-1)Final (mol L-1) | |2SO 2.001.500.5000.590 | |2O 1.501.250.0000.045 | |3SO 3.003.500.3500.260 Find the equilibrium constant for each experiment. Comment on the result. WorkbookPage 82 2( ) 2( ) 3( )2 2 99g g gSO O SO H KJ + A = 5.Effect on K if a change in temperature occurs. The following results were collected for the following reaction, Substance Experiment 1 (200oC)Experiment 2 (500oC) Initial(mol L-1) Final(mol L-1) Initial(mol L-1) Final(mol L-1) 2SO 2.001.502.002.45 2O 1.500.501.501.95 3SO 3.003.503.002.55 Find the equilibrium constant for each experiment. Comment on the result. WorkbookPage 83 Activity 5 Acids and bases In semester one we discussed (and performed) neutralisation reactions.Recall:Acid Base Salt Water + + . But what is an acid and base? Your task: In groups answer the following questions. 1.What is an acid? List some properties of acids. 2.Name three acids and describe where they may be used (other than a laboratory). 3.What is a base? List some properties of bases. 4.Name three bases and describe where they may be used. WorkbookPage 84 5.The pH scales measures how acidic or basic a substance is. Draw the pH scale and indicate where substances maybe acidic, basic or neutral. 6.Is there a pOH scale? If so, draw and label the pOH scale. 7.Is it possible for a substance to be described as both acidic and basic? Explain. WorkbookPage 85 REVIEW SET QUESTIONS The following section contains extra questions to complete in your own time. It is suggested to complete them before tests or the exam to review your understanding of the concepts of each topic of study. Answers to review sets can be found on the portal (elearning.bradford.edu.au) at various times throughout the semester. PRACTICE EXERCISES - ENERGY 1.When gaseous propane burns, it can provide heat for cooking or heating a house. a.What type of process is this and what will be the sign of AH? b.If thisprocessoccurred under standard conditionswhat namewould begivento the enthalpy change? c.Write a chemical equation for the process. 2.Consider the following reaction: 2CH3OH(l)+3O2(g) 4H2O(l)+ 2CO2(g) AH = - 1452.8kJ What is the value of AH if ..... a. the equation is multiplied throughout by 2. b.the direction of the reaction is reversed so that the reactants become products. c. water vapour instead of liquid water is formed as the product. (AH0 of vaporisation for water=+44.0 kJ mol-1) 3.Inindustry methane isconverted into methanol for useas a raw material in other processes. The equation for this reaction is shown below: CH4(g) + H2O(l) CH3OH(l) + H2(g) Calculate the enthalpy change for this reaction, using the data below: CH3OH(l) + 1 O2(g) CO2(g) + 2 H2O(l) H = -725 kJ 2 H2(g) + O2(g) 2 H2O(l) H = -570 kJ CH4(g) + 2 O2(g) CO2(g) + 2 H2O(l) H = -851kJ WorkbookPage 86 PRACTICE EXERCISES - HYDROCARBONS 1.Give the systematic name for the following compounds

2.Write balanced equations for the complete combustion in oxygen of methane, propane, butane and octane. 3.Define the term structural isomer. Which of the following compounds are isomeric? a.CH2=CHCH(CH3)2 b.CH3 - CH=CH - CH2CH3 c.CH3 - CH2- CH(CH3)2d.CH3 - CH = CH - CH2 - CH2- CH3 4.Draw Lewis diagrams for ethane, ethylene (ethene), and acetylene (ethyne). 5.Explain the difference between a saturated hydrocarbon and an unsaturated hydrocarbon. Give an example of each and write an equation for a typical reaction of each. PRACTICE EXERCISES ORGANIC CHEMISTRY 1.a.Draw structural formulae for the two common isomers of molecular formula C3H6O b.Which of the following are isomers? i.CH3 COOCH3ii.CH3CH2COOHiii.CH3CH2 COOCH3iv.HCOOCH2CH3 c.Name each of the above compounds 2.Givethenameandstructuralformulaofthefunctionalgroupfor(a)thealcohols,(b)the amines, (c) the organic acids, (d) the ketones, (e)the aldehydes, (f) the esters 3.Givethename,molecularandstructuralformulaefortheproductsofeachofthefollowing reactions. a.1-butanol and acidified potassium dichromate b.methanol and propanoic acid c.HCl and ethene (ethylene) 4.Which of the alcohols methanol, 1-propanol, 1-pentanol & 1-heptanol a.is the most soluble in water? b.would burn? c.has the highest boiling point? CHHHCHCH3CHCCHHH HH HCCH3HHCHHC CBrHCHHHC2H5CCH3HHHCCH3HCH WorkbookPage 87 5.Give the names and structural formulae for 6 structural isomers with the molecular formula C5H10O2 6.Write fully balanced equations for the preparation of 2-propanol from(a) 2-chloropropane (b) propene (propylene). 7.Draw the structural formula for a polymer formed from propene monomers and indicate a repeating unit. Is this an addition or condensation polymer? PRACTICE EXERCISES RATES OF REACTION 1.Make a list of all the factors that may affect the rate of a reaction and explain each one. 2.Whenacidifiedhydrogenperoxideisaddedtoasolutionofpotassiumiodide,iodineis formed. a.Write a balanced equation for this reaction. Theconcentration of iodinerisesfrom 0 to 10-5Min10 seconds.(At thisconcentration using a starch indicator the blue colour appears.) b.Calculate the average rate of reaction. 3.Hydrogen peroxide in aqueous solution is quite stable. When a small amount of manganese (iv) oxide is added to H2O2(aq), there is a brisk effervescence. A similar result is observed if a drop of fresh blood is added to H2O2(aq). Explain what causes the effervescence, and what role is played by the MnO2 and blood. 4.Whatisacatalyst?Givetwoexamplesofinorganiccatalystsandhowtheyareused. What makes enzymes different from other catalysts? PRACTICE EXERCISES - EQUILIBRIUM 1.Define equilibrium. Give THREE examples of dynamic equilibria. (not necessarily chemical). 2.The equilibrium constant for the reaction2HCl(g)H2(g) + Cl2(g)

is 4.17 x 10-34 at 250C. What is the equilibrium constant for the reaction H2(g) + Cl2(g)2HCl(g)at the same temperature? 3.Write equilibrium expressions for the following reactions a.NO(g)+ O2(g)NO2(g) b.N2(g)+3H2(g) 2NH3(g) c.4NH3(g) +5O2(g)4NO(g) +6H2O(g)

WorkbookPage 88 4.For the hypothetical reaction A + 2B3C an equilibrium mixture contains 2.0 mole of A, 3.0 mole of B and 6.0 mole of C in a 2.00L vessel at 250C. Calculate a.the value of Kc at 250C, and b.the initial concentrations of A and B, if no C were present initially 5..What effect would each of the following changes have on the equilibrium concentration of ammonia in the reaction below. Explain each one using Le Chateliers Principle. 4NH3(g)+5O2(g) 4NO(g)+6H2O(g)AH = -900kJ a.an increase in temperature? b.a decrease in total pressure? c.addition of some more water vapour? d.addition of a suitable catalyst (eg. a hot platinum wire)? PRACTICE EXERCISES ACIDS AND BASES 1.Define an acid. Which of the following could behave as an acid? a.NH4Clb. Ca(OH)2c. H2SO4 d. NO3-

2.Write balanced equations for the reaction of dilute nitric acid with a.magnesium b.calcium carbonate c.potassium hydroxide d. iron(II) oxide. 3.Write equations for the ionization of sulphuric acid in two steps. Why is sulphuric acid said to be diprotic? 4.What products (names and formulae) would you predict for the following pairs of reactants? a.Sulphuric acid and sodium oxide b.Potassium hydroxide and phosphorus oxide (P4O10) 5.ThepHofthestomachisapproximately2.Whatdoesthismean? 6.Calculate the pH of the following solutions:a.0.0500MHCl(aq) b.0.0500MCa(OH)2(aq) c.0.100MHA(Ka=2.0 x 10-5) 7.What volume of 0.0100 M NaOH is required to neutralise completely 100ml of nitric acid of pH = 1.05? 8.Potassium hydroxide is a strong base. What is its conjugate acid? Is this a strong acid? 9.Writeanionicequationfortheneutralisationreactionbetweensulphuricacidandsodium hydroxide. Identify the spectator ions. WorkbookPage 89 ASSIGNMENTS -Check the timetable in the theory booklet for due dates for assignments. Assignments form 10% of the overall assessment. -Assignments should be typed and submitted to the lecturer or placed in the assignment box on Level 2 132 Grenfell Street before 4pm. Assignments must be submitted with a completed cover sheet. -Assignments must be submitted before or on the due date. Late assignments will be awarded a 10% deduction per day late or receive a 0 mark in accordance with the academic policy. Extensions will not be granted for medical reasons unless a medical certificate is provided. -Assignments must be completed by each student individually, and there should be no copying of work by another student. -If material is copied directly from a text, website or other reference this should be acknowledged using Harvard referencing. It is permissible to paraphrase material from any of these sources, but the source should still be acknowledged. -Assignments will usually be marked and returned within 2 weeks of the due date. WorkbookPage 90 ASSIGNMENT6 - Energy (Total marks 29) 1.The following enthalpy values refer to CF4 a gas at room temperature. C(s) +2F2(g) CF4(g) AH = - 925 kJmol-1 CF4(s) CF4(g) AH = + 15 kJmol-1 (a)Explainthesignificanceofthedifferenceinsignandthelargedifferencein size of these AH values.(2 marks) (b)Is CF4(g)likely to be chemically stable at room temperature? Explain.(2 marks) (c)What is the name of the change from solid to gas?(1 mark) (d)What would be standard conditions for the first reaction?(2 marks) 2.The enthalpy of solution of anhydrous sodium nitrate is +21 kJmol-1. a.Explain the meaning of this statement. (2 marks) b.Write the appropriate thermochemical equation for this process.(2 marks) c.Draw and label an energy profile diagram of the reaction. (3 marks) d.Describe the 2 main energy processes involved in the dissolving of sodium nitrate in water.(4 marks) e.A solution was prepared by adding 3.42g of anhydrous sodium nitrate to 100mL ofwater.Theinitialtemperatureofthewaterwas18.50C.Determinethefinal temperature of the solution.(4 marks)

3.Itisnotpracticaltomeasuretheenthalpyofformationofethanoldirectly,butthe standardenthalpiesofcombustionforcarbon(graphite),hydrogenandethanolhave beenmeasuredbycalorimetryandfoundtobe394kJmol-1,286kJmol-1and386kJmol-1respectively.Usethesevaluestodeterminethestandardenthalpyof formation of ethanol.(4 marks) 4.Explain why it is dangerous to add water to a concentrated acid such as sulphuric acid inadilutionprocess. You should always add acid to water!(Hint:theacidreacts exothermically with the water)(3 marks) WorkbookPage 91 ASSIGNMENT 7 Hydrocarbons and alcohols(Total marks 37) 1.Writethenameandstructuralformulaofallthecompoundswiththemolecular formula C5H10. (6 marks) 2.Draw the structural formulae for the following compounds a.1-chloro-3-methyl-hexane b.2, 2-dimethyl-3-heptene c.2 - butyne d.2 pentanol e.3, 4- dimethyl -1- octanol(10 marks) 3.Write balanced equations for each reaction below (include the conditions under which the reaction would occur) and state the type of reaction that occurs. a. ethane with chlorineb.1-butene with bromine c.propene with water d.2-butene with hydrogen e.ethyne with chlorine f.2-pentanol with acidified potassium dichromate(12 marks) 4.Explainthedifferencebetweenaprimary,secondaryandtertiaryalcohol.Givean example of each and discuss how they are oxidised. (6 marks) 5.Somebottlesofvodkahavethephrasetripleddistilledonthelabel.Explainthe reason why vodka is distilled (include a diagram).(3 marks) WorkbookPage 92 ASSIGNMENT 8- Organic chemistry(Total marks 35) 1.Writefullbalancedequationsshowinghowyouwouldconvertethanoltoethyl acetate using no other organic compounds.(4 marks) 2.Give systematic names for the following compounds a.b.c.

d.e.f.

g.h.i. (9 marks) 3.Lauric acid (dodecanoic acid), a white solid at room temperature and insoluble in water, has the following structureCH3(CH2)10COOH. Cetyl alcohol (1-hexadecanol) a white solid at room temperature and insoluble in water has the following structure CH3(CH2)15OH. Describe and explain, with the aid of equations, how the reagents sodium carbonate solution and hydrochloric acid could be used to obtain separate pure samples of cetyl alcohol and lauric acid from a mixture of the two substances.(4 marks) 4.The cleaning action of sodium stearate soap (C17H35COONa) is very much reduced in acid solutions, because the soap anions form stearic acid. a.Write an equation to represent the formation of stearic acid from sodium stearate. b.Why are stearic acid molecules not as effective in cleaning as stearate ions. (3 marks) 5.The repeating unit for a particular nylon can be represented as -CO(CH2)8CONH(CH2)5NH-. a. Draw the structural formula for a section of this polymer showing at least 2 repeating units. Indicate one repeating unit using square brackets.b. Name and draw the structural formulae for the monomers used to make this polymer. (4 marks) CH CH2 CH2 CH3OCH3 CH2 CH2 CH CH3OHOCH3CH2 CH2C OH OCH3CH2 C CH2 CH3 OCH3 CH2 CH2COCH2 CH3CH3CH2 NH2CH3 CH CH2CH2 CH2OH CH3 CH2CH2 C CH2CH2 CH3CH3CH3ClCH3CH CH3NH2 WorkbookPage 93 6.A mixture of compound A (C10H21COOCH3), a colourless liquid, and excess sodium hydroxide solution was heated under reflux for 3 hours. The reaction mixture was then distilled until 10mL of distillate had been collected. The reaction mixture was then cooled and acidified with excess hydrochloric acid. A white precipitate formed which was filtered and washed with cold distilled water. The distillate was redistilled collecting the fraction between 630C and 660C. i.Name any functional groups present in A.(1 mark) ii.What observation would lead you to decide that the reflux reaction was complete?(1 mark) iii.Write balanced equations for the reactions which occur during reflux and in forming the white precipitate. (2 marks) iv.Name the white solid formed following addition of HCl.(1 mark) v.Name the liquid which was distilled off between 630C and 660C and any functional groups it contains.(2 marks) vi.Write an equation to show what happens if a lighted match is placed near a sample of the distillate.(2 marks) vii. Explain why one of the final products is soluble in water and the other not. (2 marks) WorkbookPage 94 ASSIGNMENT 9 Rates of reaction(total marks 34) 1.Tworeactionsareperformedonmarblechips(calciumcarbonate),(inexcess)with hydrochloricacidofdifferentconcentrations.Thevolumeofcarbondioxidegas evolved in each experiment is collected in a syringe and measured at regular intervals. Experiment 1 Volume (ml)8.526.552.588.5 Time (s)13610 Experiment 2 Volume (ml)0.523.036.054.0 Time (s)25812

a.Plot the experimental results on the same graph (volume versus time).(3 marks) b.Usethegraphtocalculatetheaveragerateofreactionforeachexperiment(ml per s)(2 marks) c.Which experiment used the more concentrated acid? Explain your answer. (2 marks) d.Write an equation for the reaction.(1 mark) 2.The formation of small amounts of nitric oxide, NO, in car engines is the first step in theformationofsmog.Nitricoxideisreadilyoxidisedtonitrogendioxidebythe reaction ( ) 2( ) 2( )2 2g g gNO O NO + The following experimental data was recorded at a particular temperature. Initial concentration (mol L-1)Rate of formation of NO2 (mol L-1 s-1) | |2O | |NO0.00100.00307.10 0.00200.003028.40 0.00100.006014.20 a.Explain how the order of each reactant is found.(4 marks) b.Determine the rate law for the reaction.(3 marks) c.What is the overall order of the reaction?(1 mark) WorkbookPage 95 3.Tin reacts with iodine dissolved in an organic solvent, to form tin (IV) iodide which is solubleinthesamesolvent.Apieceoftinsheetissuspendedfromthehookofan analytic balance with a nylon thread. As the reaction proceeds the tin loses mass. The experimentisperformedwithdifferentconcentrationsolutionsofiodine,anddata recorded for each. The data is listed below. Apparent Mass of Tin Square (Grams) Time (min) Saturated I280% I260% I240% I2 00.47950.46060.44600.4345 20.47810.45920.44480.4334 40.47630.45770.44360.4318 60.4739data missed0.44220.4313 80.47220.45450.44090.4300 100.47000.45290.44000.4290 120.46780.4521data missed0.4285 140.46640.45040.43810.4282 160.46460.44900.43690.4264 180.46230.44800.43570.4262 200.46090.44600.43480.4257 a.Using the same axes, plot the mass loss of tin against time for each concentration of I2.(4 marks) b.Calculate the slope of each line (which is the rate of the reaction).(4 marks) c.On another graph plot the rate (g/min) against concentration.(3 marks) d.What relationship is there between rate and concentration?(2 marks) e.What conclusions can be made about the rate order? (1 mark) f.Describe and explain the effect on the rate of reaction ofi.using powdered tin. ii.performing the reaction at a higher temperature.(4 marks) WorkbookPage 96 ASSIGNMENT 10 Equilibrium(total marks 30) 1.The formation of the diamine silver (I) ion, Ag(NH3)2+, in aqueous solution can be represented by the following equilibrium: Ag(H2O)2+(aq)+2NH3 (aq)Ag(NH3)2+(aq) +2H2O(l) a.In an equilibrium mixture, the concentration of Ag+ (Ag(H2O)2+), NH3, and Ag(NH3)2+ are 0.0067M, 10-3M and 0.10M respectively. Calculate the equilibrium constant for this reaction.(3 marks) b.If sodium chloride solution is added a solid precipitate (AgCl) forms. If the temperature remains constant explain the effect on i.the value of Kc ii.the position of the equilibrium. (4 marks) 2.The commercial preparation of sulphuric acid by the Contact Process involves the catalytic oxidation of sulphur dioxide to sulphur trioxide. a.Write a chemical equation for this equilibrium.(1 mark) b.Write an expression for Kc.(1 mark) c.If AH of reaction for the formation of 1 mole of SO3(g)from sulphur dioxide and oxygen is -99 kJ, explain why i.the reaction is carried out at a comparatively low temperature (4500C is a low temperature in industry),ii.excess oxygen (more than the stoichiometric quantity) is added. iii.the reaction is not carried out at a much lower temperature? (6 marks) 3.Ammonium carbonate has a tendency to decompose: (NH4)2 CO3(s) 2NH3(g) +CO2(g) +H2O(g)

Use le Chatelier's principle to predict the amount of decomposition when a.the solid is stored in an airtight container with very little air space above the solid. b.the solid is stored in an open container c.the solid is stored in an open container in a closed desiccator, above some fused calcium chloride (a drying agent).(6 marks) WorkbookPage 97 2( ) 2( ) 3( ) ( ) g g g gSO NO SO NO + + 4.A 2.00 L flask was filled with 4.00 mol L-1 of gaseous SO2 and 3.00 mol L-1 gaseous NO2 and heated. Equilibrium was reached after 10 minutes and it was found 1.30mol L-1 gaseous NO was present. The equation for the reaction is a.Calculate the value of Kc for this reaction.(4 marks) b.Draw a graph of the concentration against time for the above reaction. (3 marks) c.Extend your graph of b. if at 15 minutes some SO3 was removed from the flask.(2 marks) WorkbookPage 98 ASSIGNMENT 11 Acids and bases(total marks 41) 1.Which of the following reactions are acid-base reactions?(6 marks) a.Ca + S CaS b.H2SO4 +H2OHSO4-+H3O+ c.H2+Cl2

2HCl d.H3O++OH-2H2O e.NH3+H2ONH4++OH- f.O2-+H2O2OH- Which of the reactants in the above equations could be amphiprotic? 2.a.Explain the difference between a strong acid and a concentrated acid.(2 marks) b.Give an example of a strong acid and a weak acid.(1 mark) 3. a.Describe the type of bonding in a molecule of hydrogen chloride.(1 mark) b.Explain why liquid hydrogen chloride does not conduct electricity but a solution of hydrogen chloride in water does. (2 marks) c.Why is the combination of hydrogen chloride with ammonia considered to be an acid-base reaction? (2 marks) 4.Write a balanced equation for the reaction of a.nitric acid and barium oxide b.Lithium hydroxide and sulphur trioxide(4 marks) 5.Calculate the pH of the following solutions:a.0.00200Mpotassium hydroxide(2 marks) b.0.00400Mperchloric acid( )4HClO (2 marks) c.1.00MHA,(Ka = 4.0 x 10-5)(3 marks) d.If 100 mLof 0.050 M hydrochloricacid solution was mixed with 150 mL of 0.0010M of calcium hydroxide.(3 marks) WorkbookPage 99 6.A small amount of 0.110 M sodium ethanoate is added to a 0.110 M ethanoic acid. a.What is this type of solution called? (1 mark) b.Write a chemical equation for this solution.(1 mark) c.What would be the effect on the pH of this solution of adding small amounts of an acid? Explain.(3 marks) d.If 51.8 10aK= , calculate the pH of the solution.(2 marks) 7.Explain, using an equation, whether following solutions are acidic, basic or neutral. (6 marks) a.sodium propanoateb.ammonium chloride c.calcium nitrate WorkbookPage 100 PRACTICAL RULES AND REPORTS LABORATORY RULES 1.Practical sessions are not held every week. Check the timetable in the theory booklet for the practical schedule. If a practical session is not allocated it will be used for an extra tutorial lesson.2.You must purchase your own safety glasses and laboratory coat.These must be worn at all times in the laboratory.If you wear prescription glasses you must have safety glasses or goggles that can be worn over your normal glasses. 3.Covered shoes must be worn in the laboratory.Open sandals and thongs are not acceptable. 4.No food or drink is permitted in the laboratory. 5.Students must work with the partner to whom they are allocated for all practical sessions. 6.Practical reports must be submitted within one week of completion of a practical normally during the next practical class. Late reports will not be accepted unless prior approval for an extension has been granted. 7.Practical reports must be submitted jointly by the two students who completed the practical together (one report per pair). Both students will receive the same mark, unless it is clear that one student is doing all the work and the other student is not contributing.If this is the case the student who is not contributing will be given zero. 8.Practical reports should be typed and submitted to your teacher or placed in the assignment box with a completed cover sheet. Practical reports form 10% of the overall assessment. PRACTICAL REPORTS The practical reports make up a substantial part of your overall mark for the year (10%) so it is expected that you put a reasonable amount of effort into your reports.As a rough guide you might expect your completed reports to be about 3 to 6 pages long, although this will vary a little depending on the nature of the practical. Tense and Language We expect your reports to be written in a standard scientific format using the PASSIVE VOICE.This means that you write in the past tense and you do not use Ior we.For example you should write: A large test tube was washed and dried before 20 mls of ethanol was added to the test tube.The ethanol was then gently warmed in a water bath set at 30C. NOT I washed and dried a large test tube and then I poured 20 mls of ethanol into the test tube.We then gently warmed the ethanol in a water bath set at 30C. The report should use formal academic English.Slang and informal language should not be used. FORMAT Your report should be set out in the following sections: WorkbookPage 101 TITLE: You should show the title of the prac, your names and the date of the practical at the top of the page. INTRODUCTION:The introduction should include a basic summary of the theory relevant to the practical. This section should include any theory that you refer to later on in your discussion section. If you copy directly from an external source of information, you should reference the source in the text using the Harvard Referencing System. AIM This should be one or two sentences that state the purpose of the practical. Examples To investigate the miscibility of various liquids in water. Or To determine the concentration of an unknown hydrochloric acid solution. REQUIREMENTS (Materials and Equipment)Here you should list all the equipment and chemicals used in the experiment. SAFETY PRECAUTIONS This should list any special safety precautions, in addition to standard laboratory procedures, that have been followed.For example: Gloves were worn when handling concentrated sulphuric acid as is highly corrosive. Or Methylene chloride was handled inside the fume cabinet as its vapour is toxic. PROCEDURE (METHOD) This section should state exactly how you went about doing the experiment so that another chemist could pick up your report and repeat the experiment using only these instructions. You should set out your procedure step by step.You can use the instructions in your booklet as a basis for this section. RESULTS (Observations and Measurements) This section should just present your raw results without any discussion or interpretation.This may include one or more of the following: -Descriptions of observations.E.g. When the solid copper sulphate was added to water it quickly dissolved to give a bright blue solution.The solution was also observed to get slightly warmer. -A table of results that may include numerical results or observations. -A graph of numerical results where appropriate. WorkbookPage 102 DISCUSSION This is where you try to interpret and make sense of your results, and discuss any errors and limitations in your data.This section should: -Show, in full, any calculations you have performed. -Identify any mathematical relationships between variables that you can determine from your results (especially from graphs). -Identify any patterns, principles or rules you deduce from your data. -Identify any anomalies (results that dont fit the pattern) and suggest any possible explanations for these. -Identify any potential sources of error in your experiment and discuss the effect they may have on the accuracy and reliability of your data. -Suggest any changes to the procedure that could be made if you were to do it again, to minimise these sources of error. CONCLUSION Here you should concisely state the final conclusion that you can draw from your results.The conclusion may be any of the following: -A numerical result (e.g. the concentration of the unknown acid is 0.345 mol/L) -A mathematical relationship (e.g. the enthalpy of combustion was approximately proportional to the number of carbon atoms in the fuel). -A pattern or trend in your data (e.g. polar substances tended to dissolve in polar solvents, while non-polar substances tended to dissolve in non-polar solvents). Remember to make sure that you conclusion is supported by your data.You must not draw conclusions that are more general or more precise than your data allows. REFERENCES You must list any references (books, journals or websites) that you have used in writing your report. You may only use a website if you are able to identify the source of the site and information in it (e.g. University of Michigan or CSIRO).This does not include anonymous sites such as Wikipedia and Ask.com. WorkbookPage 103 PRACTICAL SEVEN-ENTHALPIES OF NEUTRALIZATION AND SOLUTION & HESS'SLAW I ntroductionYour introduction should cover the following points -Explain why heat changes occur in chemical reactions. -Explain the terms exothermic andendothermic -What are the standard conditions for a thermochemical reaction. -Define enthalpy of neutralisation and provide an equation as an example. -Define enthalpy ofsolution and provide an equation as an example. -Explain with the use of an equation how enthalpy changes can be calculated for thermochemical reactions in solution. -Define Hesss Law AimTocalculatetheenthalpyofneutralizationforanumberofdifferent acid - base combinations. To calculate the enthalpyof solution for potassium nitrate and sodium hydroxide. Tocalculatetheenthalpychangefortheconversionofanhydrous copper sulphate to hydrated copper sulphate using Hesss Law. RequirementsEquipment 2 polystyrene cups Cardboard lid Spatula Electronic balance Thermometer 2 100 mL measuring cylinders watchglass Chemicals Sodium hydroxide solution (2M) Hydrochloric acid solution (2M) Nitric Acid (2M) Potassium hydroxide solution (2M) Potassium nitrate solid Sodium hydroxide solid Anhydrous copper sulphate solid Hydrated copper sulphate solid Procedure 1.Construct a calorimeter from the cups as shown. 2.Useameasuringcylindertoadd50mLofHCltothecalorimeter.Recordthe temperature. 3.Rinse and dry the measuring cylinder. Measure 50 mL of sodium hydroxide and add to theacidinthecalorimeter.Stirwiththethermometerandrecordthehighest temperature reached. 4.Repeat for another acid-base combination. 5.Calculate the mass of 0.100 mol of potassium nitrate (KNO3). 6.Weigh out 0.100 mol of potassium nitrate using awatch glass. 7.Add 100 mL of water to the polystyrene cup (calorimeter) and record the temperature. 8.Quickly add all the potassium nitrate, stir with the thermometer to dissolve and record the lowest temperature reached. WorkbookPage 104 9.Repeatwith0.100molofsodiumhydroxide(NaOH).Recordthemaximum temperature reached. 10.Weigh out 5 g of anhydrous copper sulphate. 11.Add 50 mL of water to the cup. Record the temperature. 12.Addthecoppersulphate,stirringwiththethermometer.Recordthemaximum temperature change. 13.Calculate the enthalpy of solution for anhydrous copper sulphate. 14.Weigh out 10g of hydrated copper sulphate. 15.Repeat steps 11 - 13 for hydrated copper sulphate. Results Record all results ie the temperature changes for all reactions and the volume (mass) of water in the reaction. For the reactions of acid + base (neutralisation) there should be 4 reactions. Make sure you record the molar masses of the copper compounds used from the reagent bottles. NaOHKNO3CuSO4CuSO4.5H2O Mass weighed (g) Molar mass(g mol-1) HCl + NaOH HCl + KOH HNO3 + NaOH HNO3 + KOH NaOH + aq KNO3 +aq CuSO4 + aq CuSO4.5H2O + aq Initial temp (oC) Final Temp (oC) T (oC) WorkbookPage 105 Calculations Use the formula AH0= ATx m(H20) x4.18 1000xn Kilo joules AT = temperature change in 0C m = mass of water in g 4.18 is the specific heat capacity of water * in joules g-10C-1 Dividing by 1000 converts the answer from joules to kilojoules n = the number of moles of substance reacting and is used to find the standard enthalpy Write equations for allreactions For steps 10 15 Rearrange the two equations to achieve the equation below. (Dont forget to change the enthalpy values where necessary) CuSO4(s) +5H2O(l) CuSO4. 5H2O(s)

Then add the altered enthalpies to find the enthalpy change for this reaction Assumptions (1)Therearenoheatlossestoorheatgainsfromtheatmosphere,thecup,the thermometer or the surroundings. (2)*For a 10C temperature change for 1g of solution 4.18 J of energy are required. Discussion -Write thermochemical equations for all reactions occurring. -Show all your working in terms ofenergy changes ( indicate the sign of the energy change). -Comment on thereason of why all the temperature changes for the enthalpy of neutralisation reactions are similar.-For the Hesss Law practical show how the calculation for the required energy change is made. Thermochemical equations for both reactions should be written and then show how they be arranged to add up to the required equation. Errors Discuss any errors that may occur in the practical and their affect on the value of H. WorkbookPage 106 PRACTICAL EIGHT -ALCOHOLS, ALDEHYDES & KETONES I ntroduction The following points should form part of the introduction to this practical -What are the functional groups for an alcohol, aldehyde and ketone (draw structures)? -Identify the structural differences between primary, secondary and tertiary alcohols. -Outline the products produced ( if any) when acidified potassium dichromate is used to oxidise a primary alcohol, a secondary alcohol, a tertiary alcohol, an aldehyde and a ketone. Indicate any colour changes that may occur. -Write a half equation for acidified dichromate acting as an oxidising agent. -Tollens test. Outline how Tollens test can be used to identify an aldehyde. Provide an example of the product formed when Tollens reagent reacts with an aldehyde.( remember the solution is alkaline). Aim -To investigate the oxidation of primary secondary and tertiary alcohols -To use acidified dichromate solution and Tollens reagent to identify alcohols aldehydes and ketones. Requirements Equipment Hot plate Thermometer Glass stirring rod Test tubes, rack and stoppers 2 250 mL beaker 10 mL pipette Chemicals Ethanol 1 Propanol 2 - Propanol 2 methyl 2- propanol Ethanal Propanone Propanal 5% Glucose solution Acidified potassium dichromate solution (0.08M) Silver nitrate solution (0.1 M) Sodium hydroxide solution (2 M) Dilute ammonia solution Unknown liquids labelled X, Y and Z

WorkbookPage 107 Procedure 1.Approximatelyhalffilla250mLbeakerwithwaterandheatto600C.Maintainthe temperature at 600C to 700C. 2.Add2mL.ofeachofthealcohols,aldehydesandketonestoseparatetesttubesand place in the water bath. 3.Add 6 drops of the acidified potassium dichromate solution to each tube and stir well (rinse the rod between stirrings). Leave 5 minutes and record your observations. 4.To confirm the results add another 3 drops of the acidified potassium dichromate solution to each tube and warm for another 3 minutes. 5.Prepare a solution of ammoniacal silver nitrate (Tollens reagent) by placing 10 drops of silver nitrate solution in a clean test tube. Add 3-4 drops of sodium hydroxide. Add 4-5 drops of dilute ammonia solution to dissolve the silver oxide precipitate. 6.Add 10 drops of ethanal, stopper and shake vigorously until a silvermirror forms. 7.Repeat steps 5 and 6 using glucose and then ethanol. 8.Using the two tests identify the unknown substances X, Y and Z, given that one is a primary alcohol, one is a ketone and one is an aldehyde. Work out the quickest way to do this. Results Reactions with acidified dichromate: SubstanceObservations Ethanol 1 Propanol 2 Propanol 2 methyl 2 propanol Propanal Ethanal (acetaldehyde) Propanone (acetone) WorkbookPage 108 Tollens Test: SubstanceObservations Ethanal Glucose Ethanol Unknowns: UnknownTollens Reagent TestAcidified dichromate solution test X Y Z Discussion For each of the reactions with acidified dichromate solution explain your observations and write half and full balanced equations for the reactions occurring. Explain your observations for the reactions with Tollens reagent.For the unknowns explain how your observations enable you to identify each of the unknowns. WorkbookPage 109 PRACTICAL NINE -ESTERS I ntroduction FORMATION: Esters are formed from the reaction of an alcohol with a carboxylic acid using concentrated sulphuric acid as a catalyst. The initial reaction for formation of the ester is carried out under REFLUX, using a vertical condenser attached to the reaction vessel (flask). Reflux enables the reaction to take place at a temperature higher than the boiling points of the reactants and products and this will increase the RATE of reaction. The condenser also collects and condenses any evaporating reactants and products and they fall back into the reaction flask. ROH +RCOOH RCOOR+ H2O The reaction is an EQUILIBRIUM reaction so that after reflux there will reactants and products present in the reaction flask. ie. alcohol, carboxylic acid, ester, water and sulphuric acid. SEPARATION: IN SEPARATING FUNNEL: 1.Add water this will remove the water soluble acid. Discard the lower layer. 2.Add solid sodium carbonate this will react with the remaining carboxylic acid changing it to soluble carboxylate ion. Then add water and discard the lower layer. 2RCOOH +Na2CO32RCOONa + CO2 +H2O 3.Transfer the upper (water insoluble) layer to a beaker. Add solid fused calcium chloride to this organic layer. The fused calcium chloride will absorb any remaining water. THE CLEAR LIQUID NOW CONTAINS THE ESTER AND THE WATER INSOLUBLE ALCOHOL. DISTILLATION ( Purification): The Ester and the Alcohol have different boiling points and can be separated by distillation. The alcohol has the lower boiling point. When distilled using a condenser the lower boiling point liquid (alcohol), will distil over first and then the higher boiling point liquid (ester) will distil over. By careful control of the temperature in measuring the temperature of the vapours, the pure sample of the ester can be collected at a temperature of 122+ degrees. The Ester should be a clear liquid with a characteristic smell. AimTo prepare and purify a sample of the ester butyl ethanoate. WorkbookPage 110 Requirements Equipment Heat plate 2 Retort stand Filter funnel Spatula 2 100 mL beakers Thermometer 10 mL measuring cylinder 50 mL measuring cylinder Separating funnel Reflux/Distillation apparatus Chemicals 1- butanol Ethanoic acid (concentrated)Sulphuric acid (concentrated) Sodium carbonate (solid) Anhydrous calcium chloride solid Boiling chips Procedure 1.Place12mLofbutan-1-ol,9mLofconcentratedethanoicacidand1mLofconcentratedsulphuricacidintherefluxflask.Addafewboilingchipsandthe condenser. 2.Heat this mixture at reflux for 30 minutes and then allow to cool for 5 minutes. 3.Pourtheesterintoaseparatingfunnelcontaining10-15mLofwater.Shakeand allow the layers to separate. Discard the lower aqueous layer. 4.Add a small amount of solid sodium carbonate until the effervescence ceases, then add water until a solution is obtained. Separate discarding the lower aqueous layer. 5.Add fused calcium chloride to dry the organic layer. 6.Decant using a small filter funnel into a pear shaped flask. Distil the product using the distillation apparatus collecting the fraction boiling between 122 - 1280 C. Results In your results outline what you observed in each of the steps involved in this preparation Discussion Your discussion should simply be a statement about the nature of your product eg colour, smell etc. WorkbookPage 111 PRACTICAL TEN-MOLECULAR MODELS I ntroduction MOLECULAR FORMULA: A formula that shows the type and number of atoms present in a molecule of that substance eg H2O, NH3 STRUCTURAL FORMAL: A formula/diagram that shows the spatial arrangement ofatoms in a molecule. e