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1
GCSE CHEMISTRY (SEPARATE)
REVISION BOOKLET
Name:…………………………………………………………………………………………………………….
P1 Summary Sheets 2 Calculations
3 Equilibrium
4 Reactivity of metals
P2
Summary Sheets 5 Ion Tests
6 Organic
7 Organic
8 Materials
P1 Calculations 9 Formulae needed
10-11 Calculation practice (1)
12-13 Calculation practice (2)
14 Core Practical - Titration
P1 Haber Process and
Equilbrium
15-16 Questions
17 6 mark question on Haber Process
18 Equilibrium question – old past paper
18-23 SS 14-16 Topic Test questions
P1 Transition metals & alloys 23-25 Questions
P2 Ions 26-27 Questions
28 6 mark question on Ion
identification
29-30 SC25-26 Topic Test questions
31-33 Quantitative analysis questions
P2 Organic Chemistry 34-38 Questions
39 Core Practical – Combustion of
alcohols.
40-44 SC22-24 Topic Test questions
45-46 Hydrocarbon questions
47-49 Alcohols and carboxylic acid
questions
50-52 Polymer questions
P2 Materials 55-57 Questions
2
3
4
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8
9
EQUATIONS TO LEARN FOR TRIPLE CHEMISTRY
Number of moles = mass in grams
Relative atomic mass (Ar) or Relative formula mass (Mr)
Number of particles = Number of moles x Avogadro’s constant
Number of moles = Concentration (in mol dm-3) x volume (in dm3)
Concentration (in g dm-3) = mass of solute (in g)
Volume of solution (in dm3)
Concentration (in mol dm-3) = moles of solute
Volume of solution (in dm3)
Rf value = Distance moved by solute
Distance moved by solvent
Relative atomic mass = (% abundance of A x atomic mass of A) + (% abundance of B x atomic mass of B )
100
Energy change of a reaction = Bond enthalpies of the reactants – Bond enthalpies of products
Percentage yield = Actual mass of product x 100
Theoretical mass of product
Atom Economy = Mr of useful product x 100
Mr of all products
Volume of a gas (cm3) = Number of moles x 24000
Remember to convert
volumes in cm3 to dm3
1 dm3 = 1000 cm3
To convert cm3 to dm3
divide by 1000
10
REVISION CALCULATION QUESTIONS (1)- TRIPLE
1. Calculating theoretical masses
Ca(OH)2 + 2HCl CaCl2 + 2H2O
If 3.2g of calcium hydroxide reacts with hydrochloric acid calculate the maximum mass of calcium chloride which can
be produced? Give the answer to 2 sig fig. (relative atomic masses: Ca=40 H =1 Cl = 35.5 O=16)
2. Calculating percentage yield
If the above reaction actually produced 4.5g of calcium chloride calculate the percentage yield.
3. Calculating atom economy
Ca(OH)2 + 2HCl CaCl2 + 2H2O (Relative atomic masses: Ca=40, Cl=35.5, O=16, H=1)
Calculate the atom economy of the above reaction.
4. Calculate concentrations in g dm-3
3.2g of sodium chloride is dissolved in 400cm3 of water. Calculate the concentration of the sodium chloride solution
in g dm-3. Give the answer to 2 significant figures.
5. Calculate concentrations in mol dm-3 (HIGHER)
5.4g of sodium chloride is dissolved in 300cm3 of water. Calculate the concentration of the sodium chloride solution
in mol dm-3. Give the answer to 2 significant figures. (Relative atomic masses: Na=23 Cl=35.5)
11
6. Calculating molar volumes (HIGHER)
Ca + H2SO4 CaSO4 + H2
If 5.5g of calcium reacted in the above equation calculate the volume of hydrogen produced. (Relative atomic
masses: Ca=40, H=1, S=32, O=16)
7. Titration Calculations (HIGHER)
NaOH + HCl NaCl + H2O
If 35cm3 of 1.5 mol dm-3 of NaOH reacts with 30cm3 of HCl calculate the concentration of HCl. (Relative atomic
masses: Na=23, O=16, H=1, Cl=35.5)
8. Titration Calculations (HIGHER)
NaOH + H2SO4 Na2SO4 + H2O
If 35cm3 of 1.5 mol dm-3 of NaOH reacts with 75cm3 of H2SO4 calculate the concentration of H2SO4. (Relative atomic
masses: Na=23, O=16, H=1, S=32)
12
REVISION CALCULATION QUESTIONS (2)- TRIPLE
1. Calculating theoretical masses
CaCO3 + H2SO4 CaSO4 + H2O + CO2
If 55g of CaCO3 reacts what mass of CaSO4 is produced ? (Relative atomic masses: Ca=40, C=12, O = 16, H =1)
2. Calculating percentage yield
If the above reaction actually produced 70g of calcium sulphate calculate the percentage yield.
3. Calculating atom economy
CaO + 2HCl CaCl2 + H2O
Calculate the atom economy of the above reaction.
4. Calculate concentrations in g dm-3
3.3g of sodium chloride is dissolved in 50cm3 of water. Calculate the concentration of the sodium chloride solution in
g dm-3. Give the answer to 2 significant figures.
5. Calculate concentrations in mol dm-3 (HIGHER)
5.4g of potassium chloride is dissolved in 50cm3 of water. Calculate the concentration of the potassium chloride
solution in mol dm-3. Give the answer to 2 significant figures. (Relative atomic masses: K=39, Cl=35.5)
13
6. Calculating molar volumes (HIGHER)
2K + H2SO4 K2SO4 + H2
If 5.5g of potassium reacted in the above equation calculate the volume of hydrogen produced. (Relative atomic
masses: K=39, S=32, O=16)
7. Titration Calculations (HIGHER)
NaOH + HCl NaCl + H2O
If 25cm3 of 2.0 mol dm-3 of NaOH reacts with 20cm3 of HCl calculate the concentration of HCl. (Relative atomic
masses: Na=23, O=16, H=1, Cl=35.5)
8. Titration Calculations (HIGHER)
2NaOH + H2SO4 Na2SO4 + H2O
If 22cm3 of 1.0 mol dm-3 of NaOH reacts with 75cm3 of H2SO4 calculate the concentration of H2SO4.(Relative atomic
masses: Na=23, O=16, H=1, S=32)
14
CORE PRACTICAL – Carry out an accurate acid-alkali titration, using burette, pipette and suitable
indicator.
Complete the table
Indicator Colour in acid Colour in alkali
Why can’t you use universal indicator?..............................................................................................................
What does concordant mean?...........................................................................................................................
What is meant by the end point?.......................................................................................................................
Why do you swirl the conical flask?...................................................................................................................
What safety precautions should you use when carrying out a titration?
............................................................................................................................................................................
Why rinse the burette and pipette with the solutions before starting the titration?.......................................
……………………………………………………………………………………………………………………………………………………………………..
List the equipment used in the titration and give its use:-
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15
HABER PROCESS AND EQUILIBRIUM
For the Haber Process, how is the rate of attainment of equilibrium affected by changes
in temperature?
For the Haber Process, how is the rate of attainment of equilibrium affected by changes
in pressure?
For the Haber Process, how is the rate of attainment of equilibrium affected by changes
in concentration?
For the Haber Process, how is the rate of attainment of equilibrium affected by using a
catalyst?
For the Haber Process how is the position of equilibrium affected by changes in
temperature?
For the Haber Process how is the position of equilibrium affected by changes in
pressure?
For the Haber Process how is the position of equilibrium affected by changes in
concentration?
16
What elements do fertilisers contain and why?
How is ammonia used in the manufacture of fertilisers?
How can ammonium sulphate be prepared in the laboratory?
How can ammonium sulphate be prepared on an industrial scale?
What does a chemical cell do?
Give the advantages of hydrogen-oxygen fuel cells
Give the disadvantages of hydrogen-oxygen fuel cells
17
The Haber Process
Gases and ammonia
The reaction between nitrogen and hydrogen is exothermic.
If nitrogen and hydrogen were reacted at 90 atm pressure and 300 °C, without a catalyst, some ammonia would be formed eventually. In the Haber process a pressure of 150 atm and a temperature of 450 °C are used, in the presence of an iron catalyst. Explain, with reasons, why the Haber process conditions are better for the manufacture of ammonia.
(6)
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EQUILIBRIUM QUESTION In industry ethanol is produced by the reaction of ethene and steam at 300°C and 60 atmospheres pressure using a catalyst. The equation for the reaction is:
C2H4 (g) + H2O (g) C2H5OH (g)
The forward reaction is exothermic. Use Le Chatelier’s Principle to predict the effect of increasing temperature on the amount of ethanol produced at equilibrium. Give a reason for your prediction.
…………………………………………………………………………………………………………………………………………
…………………………………………………………………………………………………………………………………….(2)
Explain how increasing the pressure of the reactants will affect the amount ethanol produced at equilibrium.
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TOPIC 14-16 SEPARATES
1 Ammonium sulfate is used as a fertiliser. It can be prepared in the laboratory or produced in a factory.
a Which of these is the correct formula for ammonium sulfate?
Tick one box.
A NH4SO4
B NH4(SO4)2
C (NH3)2SO4
D (NH4)2SO4 (1)
b Give one difference between preparing ammonium sulfate in a laboratory and producing it in a factory.
___________________________________________________________________________________
_______________________________________________________________________________ (1)
2 A student carries out titrations to find the concentration of some dilute sulfuric acid. The student adds 25.00 cm3 of
sodium hydroxide solution to a conical flask, then a few drops of indicator. He adds dilute sulfuric acid from a
burette until the end-point is reached.
a Which of these is most suitable for measuring 25.00 cm3 of sodium hydroxide solution? Tick one box.
A measuring cylinder
B beaker
C pipette
D conical flask (1)
b Universal indicator is a common acid–alkali indicator.
i Suggest a reason why universal indicator solution is not suitable for use in this titration.
________________________________________________________________________________
(1)
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ii Name a suitable indicator for this titration.
________________________________________________________________________________
(1)
iii State the expected colour change at the end-point for the indicator named in part (ii).
________________________________________________________________________________
(1)
c The table shows the student’s results.
Titration 1 Titration 2 Titration 3 Titration 4
final burette reading (cm3) 24 46.10 22.70 44.90
initial burette reading (cm3) 2 24.00 0.00 22.70
volume of acid used (cm3) 22 22.10 22.70 22.20
i Two of the titrations 1–4 should not be used to calculate the mean of the volume of acid. Identify these two
titrations. For each one, give a reason why it should not be used in the calculation.
Titration number ___________________________________________________________________
Reason__________________________________________________________________________
Titration number ___________________________________________________________________
Reason_____________________________________________________________________ (3)
ii Calculate the mean volume of acid used to neutralise the sodium hydroxide solution. In your calculation,
do not include the titrations identified in part (i).
mean volume = ____________________ cm3 (2)
d In another experiment, dilute sulfuric acid is titrated with a 0.100 mol dm–3 sodium hydroxide solution:
2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l)
26.60 cm3 of dilute sulfuric acid is needed to neutralise 25.00 cm3 of this sodium hydroxide solution.
Calculate the concentration of the dilute sulfuric acid in mol dm–3.
concentration of sulfuric acid = ____________________ mol dm−3 (4)
20
3 Ammonium nitrate, NH4NO3, is used as a fertiliser.
a 0.10 mol of ammonium nitrate is dissolved in 50 cm3 of water. Calculate the concentration of the solution
formed in mol dm–3.
concentration of ammonium nitrate solution = ____________________ mol dm–3 (2)
b Calculate the relative formula mass of ammonium nitrate.
(relative atomic masses: H = 1, N = 14, O = 16)
relative formula mass = ____________________(1)
c Use your answers to parts a and b to calculate the concentration of the ammonium nitrate solution in
g dm–3.
concentration of ammonium nitrate solution = ____________________ g dm–3(1)
4 Ammonia, NH3, can be prepared by heating a mixture of calcium hydroxide and ammonium chloride.
a The theoretical yield in a reaction is 2.40 g. The actual yield is 2.10 g. Calculate the percentage yield.
percentage yield = ____________________(2)
b Give two reasons why the actual yield is usually less than the theoretical yield.
1 _________________________________________________________________________________
___________________________________________________________________________________
2 _________________________________________________________________________________
________________________________________________________________________________ (2)
c A teacher prepares some ammonia. An excess of calcium hydroxide is heated with 0.615 g of
ammonium chloride:
Ca(OH)2(s) + 2NH4Cl(s) → CaCl2(s) + 2H2O(l) + 2NH3(g)
i Calculate the amount, in mol, of ammonium chloride used. (relative formula mass of NH4Cl = 53.5)
ammonium chloride used = ____________________ mol(1)
21
ii Use your answer to part (i) to calculate the maximum volume of ammonia that could be formed.
(One mole of any gas occupies 24 dm3 at room temperature and pressure.)
maximum volume of ammonia = ____________________ dm3 (1)
d Calculate the atom economy of the reaction. Give your answer to 3 significant figures.
(relative formula masses: Ca(OH)2 = 74, NH4Cl = 53.5, NH3 = 17)
atom economy = ____________________(3)
5 Sulfuric acid and ammonia are used in the manufacture of fertilisers. The contact process is used to produce
sulfur trioxide, SO3, and is one of the stages involved in the manufacture of sulfuric acid:
2SO2 + O2 ⇌ 2SO3
a The pressure used in the contact process is about 2
atmospheres.
i Predict the effect of increasing the pressure on the equilibrium position. Give a reason for your answer.
________________________________________________________________________________
_____________________________________________________________________________ (1)
ii Predict the effect of increasing the pressure on how quickly equilibrium is reached.
________________________________________________________________________________
_____________________________________________________________________________ (1)
b Ammonia is manufactured using the Haber process:
N2(g) + 3H2(g) ⇌ 2NH3(g)
i Calculate the maximum volume of ammonia that can be manufactured from 100 dm3 of nitrogen and an
excess of hydrogen. Assume that the temperature and pressure remain constant.
maximum volume of ammonium = ____________________ dm3 (1)
ii The equilibrium yield of ammonia increases if the temperature is decreased. Explain why a low
temperature is not used in the Haber process.
________________________________________________________________________________
____________________________________________________________________________ (2)
22
iii Iron is used in the Haber process. Predict its effect on how quickly equilibrium would be reached, and give
a reason that explains your answer.
________________________________________________________________________________
________________________________________________________________________________
________________________________________________________________________________
_____________________________________________________________________________ (2)
6 Chemical cells and fuel cells use chemical reactions to produce a voltage.
a Silver oxide chemical cells are used in watches. A voltage is produced when zinc reacts with silver oxide. The
voltage of these cells decreases when they are in use. Give a reason why.
________________________________________________________________________________ (1)
b Some electric vehicles use fuel cells. Hydrogen or ethanol, C2H5OH, may be used as the fuel in fuel cells. The
overall reactions that take place are the same as in complete combustion. Compare and contrast the use of
hydrogen and ethanol in fuel cells.
___________________________________________________________________________________
___________________________________________________________________________________
___________________________________________________________________________________
________________________________________________________________________________ (3)
7 Epoxyethane, C2H4O, is an important industrial substance. Around 17 million tonnes are manufactured
each year, mainly as a feedstock for making engine coolants and polyesters.
There are two industrial pathways to manufacture epoxyethane.
Pathway 1
Ethene reacts with chlorine and calcium hydroxide in two complex stages.
The overall reaction is: C2H4 + Cl2 + Ca(OH)2 → C2H4O + CaCl2 + H2O
For every tonne of epoxyethane manufactured, about 200 kg of hazardous chlorine compounds also form as by-
products. Chlorine is a toxic gas that is expensive to manufacture.
Pathway 2
Ethene reacts with oxygen from air, in the presence of a silver catalyst, in one stage.
The reaction is: C2H4 + ½O2 → C2H4O
Carbon dioxide and water also form as by-products.
The table shows some other features of these two pathways.
Pathway Atom economy Yield (%) Temperature (°C) Pressure (MPa)
1 25.4% 80 100 0.2
2 100% 80 250 2
23
Evaluate the two pathways for making epoxyethane. In your answer, use your scientific knowledge and the
information given to you in the question.
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____________________________________________________________________________________ (6)
TRANSITION METALS AND ALLOYS
Give 4 properties of transition metals
What does oxidation of metals result in?
Give 3 ways to prevent rusting of iron
Give 2 uses of electroplating
24
Why is an alloy stronger than a pure metal?
Why is the alloy steel produced?
Give a use of aluminium and link to its properties
Give a use of copper and link to its properties
Give a use of gold and link to its properties
Give a use of magnalium (an alloy of aluminium and magnesium) and link to its properties
Give a use of brass (an alloy of copper and zinc) and link to its properties
QUESTION FROM THE SS9-13 HIGHER PAPER
1 This question is about metals and corrosion.
a State a typical chemical property of a transition metal.
________________________________________________________________________________ (1)
25
b Which property of aluminium allows a sheet of aluminium to be pressed into cans? Tick one box.
A It is ductile.
B It is a good conductor of electricity.
C It has a low density.
D It is malleable. (1)
c Give a reason why stainless steel instead of iron is used to make cutlery.
________________________________________________________________________________ (1)
d A steel spoon is electroplated with silver using the apparatus shown in the diagram below. Label the diagram
in the spaces provided.
(3)
e Objects made from iron and steel rust when they are in contact with air and water.
i Give the name of the metal that is used to galvanise iron to prevent it from rusting.
_____________________________________________________________________________ (1)
ii Explain how attaching blocks of magnesium to the hull of a steel ship prevents it from rusting.
________________________________________________________________________________
_____________________________________________________________________________ (2)
f Magnalium is an alloy of aluminium and magnesium and it is used to make aircraft parts. Suggest a reason
why magnalium is more suitable than pure aluminium for making aircraft parts.
________________________________________________________________________________ (1)
26
IONS
Why must ions tests be unique?
What is the flame colour of lithium ions?
What is the flame colour of sodium ions?
What is the flame colour of potassium ions?
What is the flame colour of calcium ions?
What is the flame colour of copper ions?
What is the colour of the precipitate when sodium hydroxide is added to aluminium ions?
What is the colour of the precipitate when sodium hydroxide is added to calcium ions?
What is the colour of the precipitate when sodium hydroxide is added to copper ions?
What is the colour of the precipitate when sodium hydroxide is added to iron (II) ions?
What is the colour of the precipitate when sodium hydroxide is added to iron (III) ions?
What is the test for ammonium ions?
What is the chemical test for ammonia?
What is the chemical test for a carbonate ion?
27
What is the chemical test for a sulphate ion?
What is the chemical test for chloride ion?
What is the chemical test for a bromide ion?
What is the chemical test for an iodide ion?
What are the advantages of using instrumental methods of analysis?
How would you use a calibration curve with a flame photometer?
28
Key Assessment Task
Ion identification
A technician found some colourless crystals of a
substance left, unlabelled, in a beaker in a laboratory.
She knew the substance was one of potassium sulfate, potassium iodide, sodium sulfate or sodium iodide. Explain how, using chemical tests, the technician could find out if the substance left in the beaker was potassium sulfate, potassium iodide, sodium sulfate or sodium iodide. You may include equations in your answer.
(6)
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SC 25-26 TOPIC TEST
1 Flame tests are used to identify metal ions in solids.
a What flame colour is observed with copper ions? Tick one box.
A white
B yellow
C blue-green
D orange-red (1)
29
b A white compound gives a red flame test colour. Name the metal ion responsible for this.
________________________________________________________________________________ (1)
2 A few drops of sodium hydroxide solution are added to two colourless solutions, X and Y. Each solution contains a
different metal ion but both produce a white precipitate. When excess sodium hydroxide solution is added, only the
precipitate formed by solution X dissolves to form a colourless solution.
Name the metals ions in:
a solution X___________________________________________________________________ (1)
b solution Y.___________________________________________________________________ (1)
3 A student puts some iron(II) sulfate solution in a test tube. She adds a few drops of dilute hydrochloric acid to the
test tube, then a few drops of barium chloride solution.
a State what the student sees when she adds the barium chloride solution.
________________________________________________________________________________ (1)
b Why is dilute hydrochloric acid needed in this test? Tick one box.
A Chloride ions are needed for the test to work.
B It removes any carbonate ions that might be present.
C The test only works if the mixture is alkaline.
D Barium sulfate is soluble in dilute hydrochloric acid. (1)
4 A student is given a solution of a sodium salt. He adds a few drops of dilute nitric acid, then a few drops of silver
nitrate solution, AgNO3(aq). A white precipitate forms.
a Name the anion detected in this test.
________________________________________________________________________________ (1)
b Explain why dilute hydrochloric acid should not be used instead of dilute nitric acid in this test.
___________________________________________________________________________________
___________________________________________________________________________________
________________________________________________________________________________ (2)
c Write a balanced equation for the reaction that produces the precipitate. Include state symbols.
________________________________________________________________________________ (2)
5 The diagram shows five emission spectra obtained from a flame photometer. The spectrum at the bottom
was obtained from a mixture of two of the other four substances.
a Explain which ions are present in the mixture.
___________________________________________________________________________________
________________________________________________________________________________ (2)
30
b The table shows readings from a flame photometer using a standard solution of lithium ions.
Concentration of Li+ ions (g dm–3)
Reading (units)
0 0.5
0.015 1.5
A solution containing lithium ions gives a reading of 1.0 units.
i Deduce the concentration of lithium ions in this solution.
____________________________________________________________________________ (1)
ii Explain one way to use a flame photometer to improve the accuracy of the concentration measurement in
part i.
_______________________________________________________________________________
_______________________________________________________________________________
____________________________________________________________________________ (2)
6 A student is given three solutions (X, Y and Z). He carries out the following tests on three portions of
each solution.
● He carries out a flame test.
● He adds a few drops of dilute hydrochloric acid, then a few drops of barium chloride solution.
● He adds a few drops of dilute sodium hydroxide solution.
The table shows his results.
Solution Flame test Hydrochloric acid added
Barium chloride solution added
Sodium hydroxide solution added
X not done no visible change white precipitate green precipitate
forms
Y lilac flame carbon dioxide
produced no visible change no visible change
Z no visible change no visible change white precipitate
no visible change
produces an alkaline
gas on warming
Give the name of:
a solution X
________________________________________________________________________________ (2)
b solution Y
________________________________________________________________________________ (2)
c the cation in solution Z.
________________________________________________________________________________ (1)
31
QUANTITATIVE ANALYSIS Questions (BRS)
Q1. Iron(III) ions, Fe3+, react with hydroxide ions in solution to form iron(III) hydroxide.
Complete the ionic equation for this reaction.
(1)
Fe3+ + 3OH– → ......................................................................
Q2. Substance X is an ammonium salt.
(i) Complete the sentence by putting a cross ( ) in the box next to your answer. A test was carried out to find which anion is present in substance X. Dilute hydrochloric acid was added to a sample of substance X. There was effervescence and the gas given off turned limewater milky. The anion present in substance X is
(1)
A carbonate ion, CO32–
B chloride ion, Cl–
C nitrate ion, NO3–
D sulfate ion, SO42–
(ii) Describe how sodium hydroxide solution can be used to show that ammonium ions are present in substance X.
............................................................................................................................................................................ ............................................................................................................................................................................ ............................................................................................................................................................................ ........................................................................................................................................................................... .........................................................................................................................................................................(2) Q3. In industry sodium carbonate is made from sodium chloride solution and calcium carbonate in the Solvay Process.Describe the test to show that calcium carbonate contains carbonate ions. ............................................................................................................................................................................ ........................................................................................................................................................................... .........................................................................................................................................................................(3) Q4. Sodium hydroxide solution is used to identify some cations present in compounds.
(i) Sodium hydroxide solution is warmed with a solution of ammonium ions. Ammonia gas is given off.
Describe the test to show the gas is ammonia.
........................................................................................................................................................................... ........................................................................................................................................................................... .........................................................................................................................................................................(2)
(ii) Sodium hydroxide solution is also used to distinguish between iron (II) ions, Fe2+ and iron(III) ions, Fe3+, in solution. You are given a solution containing iron(II) ions and another solution containing iron(III) ions. Describe what is seen when sodium hydroxide solution is added to each of these solutions.
............................................................................................................................................................................ ........................................................................................................................................................................... .........................................................................................................................................................................(2)
Q5. Qualitative tests are used to identify ions.
32
A student carries out a flame test on an unknown solid. A red flame is seen. The students concludes that the soldi is lithium carbonate. Explain why this conclusion is not justified.
............................................................................................................................................................................ ........................................................................................................................................................................... .........................................................................................................................................................................(2)
Q6. Aluminium ions, Al3+, react with hydroxide ions in solution to give a white precipitate of aluminium hydroxide.
Write the ionic equation for this reaction. ..............................................................................................................................................(3) Q7. Sodium sulfate is tested to show the ions present in it.
The sodium sulfate is dissolved in water to make a solution.
Describe how to show that sulfate ions are present in this solution.
............................................................................................................................................................................ ........................................................................................................................................................................... .........................................................................................................................................................................(3)
Q8. The following tests were carried out on a substance containing two ions.
1. A flame test on the solid substance produced a yellow colour.
2. Dilute hydrochloric acid was added to a solution of the substance followed by a few drops of barium chloride solution. A white precipitate formed. Give the name and formula of the substance.
(2)
Name of substance ...........................................................................................................................
Formula of substance ........................................................................................................................
Q9. A technician had two bottles containing solid salts. One bottle contained a potassium salt and the other contained a sodium salt. Unfortunately the labels had fallen off the bottles. The technician tested the salts to find the ions present.
(i) Complete the sentence by putting a cross ( ) in the box next to your answer.
Both salts contained the same anion. A solution of one salt was made and some dilute nitric acid was added. Drops of silver nitrate solution were added. A yellow precipitate formed. This test shows the anion in the salt is(1)
A bromide, Br−
B chloride, Cl−
C iodide, I−
D sulfate, SO42−
(ii) The technician wanted to find out which bottle contained the sodium salt and which bottle contained the potassium salt.Explain how the technician should do this.
............................................................................................................................................................................ ........................................................................................................................................................................... .........................................................................................................................................................................(2)
33
Q10. When sodium hydroxide solution is mixed with a solution containing copper ions, Cu2+, copper hydroxide, Cu(OH)2, is formed.
(i) Describe what you would see when these solutions are mixed.
............................................................................................................................................................................ ........................................................................................................................................................................... .........................................................................................................................................................................(2)
(ii) Write the ionic equation for this reaction.
.............................................................................................................................................
(3) Q11.(a) Three solids, A, B, and C, are analysed.
(i) Solid A is potassium iodide. A small amount of solid A is dissolved in water to form a solution. Describe the test to show that the solution of A contains iodide ions.
(2) ............................................................................................................................................................................ ........................................................................................................................................................................... .........................................................................................................................................................................(2)
(ii) Solid B is ammonium chloride. Describe the test to show that solid B contains ammonium ions.
. ............................................................................................................................................................................ ........................................................................................................................................................................... .........................................................................................................................................................................(3)
(iii) Solid C is dissolved in water. When sodium hydroxide solution is added to the solution of C, a red-brown
precipitate is formed. Complete the sentence by putting a cross ( ) in the box next to your answer. This test shows that the ion present in solid C is
(1)
A copper, Cu2+
B iron(II), Fe2+
C iron(III), Fe3+
D sodium, Na+
(b) Sodium hydroxide solution can be used to test for aluminium ions and for calcium ions in solution.
Describe the results of these tests for aluminium ions and for calcium ions, explaining how the results distinguish between the two ions.
............................................................................................................................................................................ ........................................................................................................................................................................... .........................................................................................................................................................................(3)
34
ORGANIC CHEMISTRY
Draw ethane, Give the formula
Draw methane. Give the formula
Draw butane. Give the formula
Draw propane. Give the formula
Why are alkanes saturated hydrocarbons?
Draw propene. Give the formula
Draw ethene. Give the formula
Draw butene. Give the formula
35
Why are alkenes unsaturated hydrocarbons?
Draw the formulae giving the reaction of ethene + bromine
How would you use bromine water to distinguish between alkanes and alkenes
What does the combustions (oxidation) of an alkane always produce? Write the balanced equation for
the oxidation of propane.
What does the complete combustion (oxidation) of an alkene always produce? Write the balanced
equation for the oxidation of ethene.
What is a polymer?
How is poly(ethene) produced?
Explain how the uses of poly(ethene) relates to its properties
36
Explain how the uses of poly(propene) relates to its properties
Explain how the uses of poly(chloroethene) (PVC) relates to its properties
Explain how the uses of poly(tetrafluoroethene) (PTFE) relates to its properties
Why are polyesters condensation polymers?
Describe the problems of disposing of polymers
Give the advantages and disadvantages of recycling polymers
Describe DNA (as a polymer)
Describe starch (as a polymer)
Describe proteins (as a polymer)
37
Give the molecular formula and displayed formula of methanol
Give the molecular formula and displayed formula of propanol
Give the molecular formula and displayed formula of butanol
Give the molecular formula and displayed formula of ethanol
What is the functional group of an alcohol?
Give the molecular formula and displayed formula of methanoic acid
Give the molecular formula and displayed formula of propanoic acid
Give the molecular formula and displayed formula of ethanoic acid
38
Give the molecular formula and displayed formula of butanoic acid
Give the functional group of a carboxylic acid
Write the balanced equation for the oxidation of ethanol
How do you produce ethanol by fermentation?
How do you produce a more concentrated solution of ethanol?
39
Core Practical: How would you investigate the temperature rise of a known mass of water by
the combustion of alcohols.
Answer
What is the practical about?
What is being changed in the experiment?
Name three control variables
What measurements would you take
How did the temperature rise relate to the number of carbon atoms in the alcohol molecules?
40
SC22-24 TOPIC QUESTIONS
1 Alkanes are hydrocarbons.
a Explain why alkanes are hydrocarbons.
________________________________________________________________________________ (2)
b The table shows some information about the first three alkanes. Complete the table.
Name Molecular formula Structure
CH4
Ethane C2H6
propane
(3)
c Another alkane has seven carbon atoms. What is the molecular formula of this alkane? Tick one box.
A C7H7
B C7H12
C C7H14
D C7H16 (1)
2 Propene, C3H6, is an alkene.
a Draw the structure of a molecule of propene. Show all the covalent bonds.
( 2)
41
b Which row is correct for propene? Tick one box.
Type of compound Type of reaction
A saturated addition
B saturated substitution
C unsaturated addition
D unsaturated substitution
(1)
c Propane and propene are both gases. You are given a sample of both gases. Describe a test to show which
gas is propane and which gas is propene.
___________________________________________________________________________________
________________________________________________________________________________ (3)
d Describe one similarity and one difference between the structures of propane and propene molecules.
___________________________________________________________________________________
___________________________________________________________________________________
________________________________________________________________________________ (2)
3. The structure of ethanoic acid is shown below.
a Draw a circle around the carboxylic acid functional group in ethanoic acid.(1)
i Give the molecular formula of ethanoic acid_______________________________________________(1)
ii Give the empirical formula of ethanoic acid________________________________________________(1)
b A strip of magnesium ribbon is added to an excess of an aqueous solution of ethanoic acid.
Write the word equation for the reaction.
___________________________________________________________________________ (2)
c Predict the names of all of the products formed when butanoic acid reacts with aqueous
sodium carbonate.
_______________________________________________________________________________ (3)
3 This question is about polymers.
42
Polymer poly(ethene) poly(propene) PTFE
Properties flexible, cheap, good
insulator
flexible, does not
shatter
tough, slippery
a Select a polymer from the table that could be used to make non-stick coatings for saucepans.
Give a reason for your choice.
___________________________________________________________________________________
___________________________________________________________________________________
________________________________________________________________________________ (2)
b A number of methods are used to dispose of waste polymers. These include placing the waste in landfill,
recycling it and burning it.
Explain a problem caused by the disposal of polymers.
___________________________________________________________________________________
___________________________________________________________________________________
________________________________________________________________________________ (2)
c Draw the structure of the monomer that was used to form the polymer shown below.
(1)
d Ethenyl ethanoate has the structure shown below.
Draw a section of the polymer formed from ethenyl ethanoate. The section should show two repeating units.
(1)
43
4 This question is about esters and polyesters.
a Methanoic acid reacts with methanol to form an ester and another product.
iii Write the equation for the reaction between methanoic acid, HCOOH, and methanol, CH3OH. Show the
structures of the reactants and the organic product.
(3)
iv Circle the ester link in the organic product in part ai.
(1)
v Explain why the reaction in part ai is a condensation reaction.
_______________________________________________________________________________
_______________________________________________________________________________
_______________________________________________________________________________
(2)
b Draw the structures of the two monomers that were used to form the polyester shown below.
(2)
5 This question is about the combustion of ethanol and butanol.
a Write the balanced equation for the complete combustion of butanol.
___________________________________________________________________________________
(3)
44
Ethanol and butanol are burned using the apparatus shown below.
The results of the experiments are shown in the table.
Alcohol ethanol butanol
Formula C2H5OH C4H9OH
Initial mass of alcohol burner + cap + alcohol (g) 156.35 152.27
Final mass of alcohol burner + cap + alcohol (g) 155.93 151.92
Initial temperature of 100 cm3 of water (°C) 20 21
Final temperature of 100 cm3 of water (°C) 51 50
Time taken (min) 9 8
Observation burned with a clean,
blue flame
burned with a yellow,
sooty flame
Evaluate this data to decide whether ethanol or butanol is the better fuel to use to heat the water.
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
______________________________________________________________________________________ (6)
45
Hydrocarbon Questions (BRS)
Q1. Hexene is an alkene that contains six carbon atoms in its molecule.
Give the molecular formula of hexene. ........................................................... (1)
Q2. Alkanes and alkenes are hydrocarbons.
The structure of a molecule of butane is shown.
Which of the following is the empirical formula for butane? (1)
A CH
B CH2
C C2H5
D C4H10
Q3. Butene reacts with steam to produce butanol.
C4H8 + H2O → C4H9OH
What type of reaction takes place between butene and steam?
A addition
B dehydration
C neutralisation
D substitution (1)
Q4. Alkenes are unsaturated hydrocarbons.
State what is meant by unsaturated. (1)
.............................................................................................................................................. Q5. Figure 5 shows some information about the alkenes, ethene and propene.
Complete the table. The structure of propene must show all covalent bonds.
(2)
46
Q6. Ethanol can be produced by reacting ethene with steam.
Write the balanced equation for this reaction. (2)
...................................................................................................................................................................... Q7. (d) Propane and propene are bubbled through separate samples of bromine water. Describe what you would see in these tests.
...................................................................................................................................................................... ...................................................................................................................................................................... ......................................................................................................................................................................(3) Q8. (a) In the laboratory this apparatus is used to crack long chain hydrocarbon molecules to form shorter chain hydrocarbon molecules.
When the experiment is complete there is a danger that water will rise up the delivery tube into the hot test tube. State what you would do to prevent this.
(1) ................................................................................................................................................................... ...................................................................................................................................................................
(b) Complete the sentence by putting a cross ( ) in the box next to your answer. The equation for a reaction that occurs during cracking is
C12H26 → C2H6 + C6H12 + X In the balanced equation, X is
(1)
A C3H8
B C4H8
C C4H10
D C6H14
(e) In industry, long chain hydrocarbon molecules are cracked to form shorter chain hydrocarbon molecules.
Explain why this process is important. (2)
................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ...................................................................................................................................................................
47
Q9. (a) Which of these is the formula of a molecule of a hydrocarbon?
Put a cross ( ) in the box next to your answer. (1)
A CH3COOCH3
B CH3CH2Cl
C CH3CH3
D CH3COOH
(c) Methane burns in oxygen to form carbon dioxide and water. Write the balanced equation for this reaction. (3)
..............................................................................................................................................
(d) Natural gas is mainly methane. A gas with similar composition, known as bio-methane, can be produced from plants grown specifically for this purpose. Describe the advantages and disadvantages of using bio-methane rather than natural gas as a source of energy.
(6) ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ALCOHOLS AND CARBOXYLIC ACID Questions (BRS)
Q1. Complete the sentence by putting a cross ( ) in the box next to your answer. Ethanol, C2H5OH, can be converted into ethanoic acid, CH3COOH. In this reaction, ethanol is
(1)
A dehydrated
B neutralised
C neutralised
D reduced
Q2.Figure 4 shows a molecule of the alcohol, ethanol.
Figure 4
Circle the alcohol functional group in Figure 4. (1)
48
Q3. Ethanol is a member of the homologous series of alcohols. The first three members of the series are
methanol CH3OH ethanol C2H5OH propanol C3H7OH Use the formulae of these molecules to explain why these alcohols are members of the same homologous series.
(2) ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... Q4.Ethanol can also be produced by fermentation. Describe how ethanol can be produced from sugar by fermentation.
(2) ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... Q5. Figure 4 shows a molecule of the alcohol, ethanol.
Figure 4
Pentanol can be oxidised to form pentanoic acid, C5H10O2.
Draw the structure of pentanoic acid, showing all covalent bonds.
(2)
Q6. Ethanol is produced by the fermentation of glucose.
Yeast is needed for the fermentation reaction.
(i) State two other conditions for fermentation.
(2) ................................................................................................................................................................... ...................................................................................................................................................................
(ii) Complete the sentence by putting a cross ( ) in the box next to your answer.
A dilute solution of ethanol can be converted to a concentrated solution of ethanol by (1)
A filtration
B fractional distillation
C dehydration
D cracking
49
(iii) Write the balanced equation for the fermentation of glucose, C6H12O6.
(2)
.............................................................................................................................................
Q7. Figure 4 shows a molecule of the alcohol, ethanol.
Figure 4
A dilute solution of ethanol is obtained by fermentation.
Explain how a more concentrated solution of ethanol can be obtained from this dilute solution.
(3) ................................................................................................................................................................... ................................................................................................................................................................... ...................................................................................................................................................................
Q8. An alcohol A, with molecular formula C2H5OH is oxidised to a compound B with molecular formula C2H4O2.
(i) Compound B is not an alcohol and is a member of another homologous series. State the name of this homologous series.
............................................................................................................................................. ………………………..(1)
(ii) Draw the structure of a molecule of compound A and a molecule of compound B, showing all covalent bonds. (2)
Compound A
Compound B
Q9. (a) Some fuels are better fuels than others. State one factor that makes a good fuel. (1)
................................................................................................................................................................... ...................................................................................................................................................................
50
(b) Bioethanol is a fuel that can be obtained from the plant, sugar beet.
(i) Bioethanol and petrol can both be used as fuels. Explain one advantage of using bioethanol produced from sugar beet, rather than petrol produced from crude oil.
(2) ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ...................................................................................................................................................................
(ii) The main component of bioethanol is ethanol. When burnt completely, ethanol, C2H5OH, reacts with oxygen to produce carbon dioxide and water. Write the balanced equation for this reaction.
(3)
..................................................................................................................................................................................
POLYMERS Questions (BRS)
Q1. The structure of a molecule of propene is
Molecules of propene can be combined to form a molecule of poly(propene).
(i) Which of these shows part of the structure of a molecule of poly(propene)?
Put a cross ( ) in the box next to your answer. (1)
51
(ii) Ropes used on boats are often made from poly(propene).
State a property of poly(propene) that makes it suitable for use as ropes on boats.
(1)
.............................................................................................................................................
(iii) State a problem caused by the disposal of poly(propene) ropes in landfill sites.
(1) ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... Q2. Figure 7 shows a molecule of each of the substances A, B and C.
Figure 7
(i) State the name of substance A.
(1)
.............................................................................................................................................
(ii) Substance B reacts with bromine in an addition reaction.
Complete the balanced equation for this reaction showing all covalent bonds. (2)
52
(iii) Substance C can be used as a monomer to produce a polymer.
Draw a diagram to show the part of the polymer molecule formed from two molecules of substance C. (2)
Q3.* Polymers are addition or condensation polymers.
Polymers can be formed by using the monomers shown in Figure 12.
Figure 12
Explain, using appropriate monomers from Figure 12, how different polymers can be formed.
(6) ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ...................................................................................................................................................................
53
Q4. Alkenes can be polymerised to make plastic for bottles. Waste plastic bottles can be recycled, burned or buried in landfill sites. Evaluate these three methods of dealing with waste plastic bottles.
(6) ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ...................................................................................................................................................................
MATERIALS
How does the size of a nanoparticle compare to an atom?
Give the key property of a nanoparticle
What risks are associated with nanoparticles?
54
SC25-26 TOPIC TEST QUESTIONS
6 Some nanoparticles are used as catalysts. They speed up reactions without being changed chemically
or in mass at the end of the reaction.
g A cube-shaped nanoparticle has side length 3 nm. Calculate its surface area to volume ratio.
________________________________________________________________________________ (3)
h Nanoparticles make more effective catalysts than powders do. Give the property that explains this.
________________________________________________________________________________ (1)
i Give one reason why some people think nanoparticles may have a risk of harm to human health.
________________________________________________________________________________ (1)
7 The table shows some typical properties of fibres. These fibres could be mixed with a polymer resin to form
a composite material. Stiff materials resist bending when forces are applied.
Fibre Tensile strength (MPa) Stiffness (GPa) Density (kg/m3)
aramid 2800 90 1400
carbon fibre 4100 150 1600
glass fibre 3500 35 2700
Identify the fibre which would be best to use for producing a strong, flexible and lightweight composite material.
Justify your answer.
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
______________________________________________________________________________________ (3)
55
8 Some people like to buy water in disposable bottles to drink during the day. Other people prefer to fill
reusable bottles with tap water and wash them thoroughly when they get home. The table shows the properties of
five materials that could be used to make reusable water bottles.
Glass Polyester Poly(ethene) Stainless steel
Aluminium
Tensile strength (MPa)
30 50 15 800 300
Thermal conductivity
low low low high high
Appearance transparent opaque translucent opaque opaque
Dishwasher safe?
yes yes no yes yes
Other properties brittle
best water
taste
tough
good water
taste
tough
slight plastic
water taste
can dent
faint metallic
water taste
dents easily
good water
taste
Evaluate the use of these materials for making a reusable water bottle.
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
______________________________________________________________________________________ (6)
MATERIALS QUESTIONS (BRS) Q1.A nanoparticle has a diameter of 25 nm. What is the diameter of this nanoparticle, in metres?
(1)
A 2.5 × 10–4
B 2.5 × 10–6
C 2.5 × 10–8
D 2.5 × 10–10
56
Q2. Silver is a metal that is often used in jewellery.
Give one property of silver that makes it a suitable material for use in jewellery.
(1)
.............................................................................................................................................
Q3. Some socks contain nanoparticles of silver. During washing some of the nanoparticles may be removed and carried away in the waste water. Explain a possible risk associated with nanoparticles in the waste water.
(2) ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ...................................................................................................................................................................
Q4. Nanoparticles have many uses. Explain why nanoparticles are often used, rather than larger particles.
(2) ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ...................................................................................................................................................................
Q5. This question is about properties of materials. Figure 6 shows some properties of steel and Kevlar®.
Figure 6
Body armour, such as a bullet-proof vest, could be manufactured using either of these materials.
Explain two reasons why Kevlar® is preferred to steel as the material for body armour.
(4) ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ...................................................................................................................................................................
57
Q6. The use of nanoparticles has increased in recent years.
(i) The length of one side of a cube of silver is 2 cm as shown in Figure 7.
Figure 7
Calculate the surface area to volume ratio of this cube of silver. (3)
surface area to volume ratio = ...........................................................
(ii) Suggest an explanation of why a given mass of silver is more effective as a catalyst when used as nanoparticles rather than in a powder form.
(3) ................................................................................................................................................................... ................................................................................................................................................................... ................................................................................................................................................................... ...................................................................................................................................................................
