AP#Chemistry#Summer#Work# - 2018 Mr.#Herring# · scientific notation worksheet #1 name_____ express each of the following numbers in proper scientific notation:

AP#Chemistry#Summer#Work#Mr.#Herring#

curtis.herring@acsk:12.org##The#work#in#this#summer#packet#reflects#the#knowledge#and#skills#you#need#to#possess#when#you#enter#this#class.##If#you#fail#to#do#the#work,#and#don’t#know#this#information#hands#down,#you#place#yourself#in#a#position#where#you#are#likely#to#struggle#and#suffer#setbacks#the#entire#year.##Please#do#not#hesitate#to#email#me#with#any#questions#you#may#have.##I#check#my#email#regularly.##Know%the%following:%Metric%System%Significant%Figures%(sig%figs)%Stoichiometry%The%following%rules:%Rules%for%Naming%Acids%Solubility%Rules%Rules%for%assigning%oxidation%umber%Common%Polyatomic%ions%Atomic%trends:%Atomic%Radii%Charges%and%Ions%(cations%and%anions)%Ionization%Energy%Electron%Affinity%Electronegativity%Some%Thermochemistry%%%Complete%the%tasks%and%problems%with%each%of%the%following%links%to%web%pages:%%http://highschoolhub.org/hub/chemistry.cfm ; http://www.chemistrycoach.com/home.htm http://www.collegeboard.com/ap/students/chemistry/index.html www.chemmybear.com % Balancing equations practice web links http://science.widener.edu/svb/tutorial/rxnbalancingcsn7.html http://www.chemistry-drills.com/balance.html #Complete#all#of#the#accompanying#worksheets#in#this#packet.##Where#required,#calculated#answers#must#contain#correct#units,#and#be#written#to#the#correct#number#of#sig#figs#using#the#rules#for#writing#sig#figs.##Failure%to%write%the%correct%units,%and/or%report%answers%to%the%correct%number%of%sig%figs%MAKES%YOUR%ANSWER%INCORRECT!!%%#%%

- 2018

SCIENTIFIC NOTATION WORKSHEET #1 NAME______________________ EXPRESS EACH OF THE FOLLOWING NUMBERS IN PROPER SCIENTIFIC NOTATION: 1. 0.000033 = _____________________ 2. 50,000. = _____________________ 3. 0.000002 = _____________________ 4. 230,000 = _____________________ 5. 465 = _____________________ 6. 236,000,000,000 = _____________________ 7. 0.000000000000236 = _____________________ 8. 48.95 = _____________________ EXPRESS EACH OF THE FOLLOWING AS COMMON NUMBERS: 9. 3.7 x 105 = _____________________ 10. 3.21 x 10-4 = _____________________ 11. 6 x 105 = _____________________ 12. 1.99 x 10-3 = _____________________ 13. 1.7 x 1012 = _____________________ 14. 8.653 x 10-17 = _____________________ PERFORM EACH OF THE FOLLOWING OPERATIONS USING SCIENTIFIC NOTATION. YOUR ANSWERS SHOULD BE ROUNDED TO THE TENTHS COLUMN IN EACH ANSWER. 15. (2.3 x 103)(4.0 x 105) = _______________________________ 16. (9.6 x 10-1)(5.2 x 102) = _______________________________ 17. (4.56 x 10-6)(3.1 x 10-3) = _____________________________ 18. (5.7 x 108)(2.3 x 10-4) = _______________________________ 19. 6.7 x 102 = 1.3 x 103 20. 1.76 x 105 = - 5.8 x 102 21. (1.3 x 105)(8.2 x 10-2) = 7.4 x 102 22. 2.56 x 104 + 4.6 x 103

PHYSICAL PROPERTY CHEMICAL PROPERTY 1. observed with senses 1. indicates how a substance 2. determined without destroying matter reacts with something else 2. matter will be changed into a new substance after the reaction

PHYSICAL AND CHEMICAL PROPERTIES AND CHANGES Name ____________________________

Identify the following as a chemical (C) or physical property (P): ______1. blue color ______8. melting point ______2. density ______9. reacts with water ______3. flammability (burns) ______10. hardness ______4. solubility (dissolves) ______11. boiling point ______5. reacts with acid ______12. luster ______6. supports combustion ______13. odor ______7. sour taste ______14. reacts with air

Identify the following as physical (P) or chemical (C) changes. _____1. NaCl (Table Salt) dissolves in water. ______9. Milk sours. _____2. Ag (Silver) tarnishes. ______10. Sugar dissolves in water. _____3. An apple is cut. ______11. Wood rots. _____4. Heat changes H2O to steam. ______12. Pancakes cook. _____5. Baking soda reacts to vinger. ______13. Grass grows. _____6. Fe (Iron) rusts. ______14. A tire is inflated. _____7. Alcohol evaporates . ______15. Food is digested. _____8. Ice melts. ______16. Paper towel absorbs water.

Physical and Chemical Changes Part A Can you recognize the chemical and physical changes that happen all around us? If you change the way something looks, but haven’t made a new substance, a physical change (P) has occurred. If the substance has been changes into another substance, a chemical change (C) has occurred.

1. An ice cube is placed in the sun. Later there is a puddle of water. Later still the puddle is gone.

2. Two chemical are mixed together and a gas is produce.

3. A bicycle changes color as it rusts.

4. A solid is crushed to a powder.

5. Two substances are mixed and light is produced.

6. A piece of ice melts and reacts with sodium.

7. Mixing salt and pepper.

8. Chocolate syrup is dissolved in milk.

9. A marshmallow is toasted over a campfire.

10. A marshmallow is cut in half.

PHYSICAL CHANGE CHEMICAL CHANGE 1. a change in size, shape, or state 1. a change in the physical and 2. no new substance is formed chemical properties 2. a new substance is formed

#2

Part B Read each scenario. Decide whether a physical or chemical change has occurred and give evidence for your decision. The first one has been done for you to use as an example.

Scenario Physical or Chemical Change?

Evidence…

1. Umm! A student removes a loaf of bread hot from the oven. The student cuts a slice off the loaf and spreads butter on it.

Physical No change in substances. No unexpected color change, temperature change or gas given off.

2.

Your friend decides to toast a piece of bread, but leaves it in the toaster too long. The bread is black and the kitchen if full of smoke.

3. You forgot to dry the bread knife when you washed it and reddish brown spots appeared on it.

4. You blow dry your wet hair.

5.

In baking biscuits and other quick breads, the baking powder reacts to release carbon dioxide bubbles. The carbon dioxide bubbles cause the dough to rise.

6. You take out your best silver spoons and notice that they are very dull and have some black spots.

7. A straight piece of wire is coiled to form a spring.

8. Food color is dropped into water to give it color.

9.

Chewing food to break it down into smaller particles represents a _________ change, but the changing of starch into sugars by enzymes in the digestive system represents a ___________change.

10. In a fireworks show, the fireworks explode giving off heat and light.

Part C: True (T) or False (F)

1. Changing the size and shapes of pieces of wood would be a chemical change.

2. In a physical change, the makeup of matter is changed.

3. Evaporation occurs when liquid water changes into a gas.

4. Evaporation is a physical change.

5. Burning wood is a physical change.

6. Combining hydrogen and oxygen to make water is a physical change.

7. Breaking up concrete is a physical change.

8. Sand being washed out to sea from the beach is a chemical change.

9. When ice cream melts, a chemical change occurs.

10. Acid rain damaging a marble statue is a physical change.

ATOMIC STRUCTURE WORKSHEET NAME __________________________________

Atoms are composed of three sub-atomic particles: the proton, the neutron, and the electron. The proton and the neutron are found in the nucleus. Electrons are found in a cloud surrounding the nucleus. The atomic number of an element is equal to the number of protons in that element. If the atom is neutral, the number of electrons (-) is equal to the number of protons (+). If the atom carries a charge, it is referred to as an ion. The charge on an ion indicates an imbalance between protons and electrons. If the ion has a positive charge, there are more protons than electrons. To find the number of electrons, you must subtract the charge from the atomic number. If the ion has a negative charge, there are more electrons than protons. To find the number of electrons, you must add the charge to the atomic number. The mass number is a whole number equal to the number of protons plus neutrons. This is because we say that protons and neutrons each have a mass of 1 amu (standardized from Carbon-12). This number is not on the periodic table. The atomic mass is the weighted average atomic mass of all the naturally occurring isotopes of an element. This number is located on the periodic table and is usually a decimal. (Remember, an isotope is an atom of the same element with a different number of neutrons; an ion is an atom of the same element with a different number of electrons.) X= element Mass number Charge A= mass number (# of protons + # of neutrons) Z= atomic number (# of protons) A - Z = # of neutrons Isotopic symbol is in this form: Atomic number Element symbol

A

X Or, you might see: X – A Example: Aluminum - 26 Z Complete the chart.

Element/Ion Atomic Number Atomic Mass Mass

Number Protons Neutrons Electrons

1 1 H

1 1 H

1+

14 7 N

3-

41 20 Ca

108 47 Ag

108 47 Ag1+

#3

Define the following:

Atomic Number _______________________________________________________________________

Mass Number _________________________________________________________________________

Atomic Mass _________________________________________________________________________

Isotope _______________________________________________________________________________

Ion ___________________________________________________________________________________

SUMMARIZE:

How do you find the number of protons for any atom?

How do you find the number of neutrons for any atom?

How do you find the number of electrons for any atom?

Isotope Name Isotope Symbol

Number of… Atomic Number

Mass Number Protons Neutrons Electrons

Argon-40

Argon-38

Bismuth-209

5726Fe

20982Pb

16 34

28 30

34 28

37 48 37

Aluminum-27

Manganese-55

20 40

11 12 11

For chemistry help, visit www.chemfiesta.com © 2002 Cavalcade Publishing – All Rights Reserved

Periodic Trends Worksheet 1) Rank the following elements by increasing atomic radius: carbon,

aluminum, oxygen, potassium. 2) Rank the following elements by increasing electronegativity: sulfur,

oxygen, neon, aluminum. 3) What is the difference between electron affinity and ionization energy? 4) Why does fluorine have a higher ionization energy than iodine? 5) Why do elements in the same family generally have similar properties?

#4

WKS001x023 © 2000 Cavalcade Publishing (http://www.cavalcadepublishing.com) All Rights Reserved

Naming Ionic Compounds

Give the name and molar mass of the following ionic compounds:

Name Molar Mass

1) Na2CO3 ____________________________________________________

2) NaOH _____________________________________________________

3) MgBr2 _____________________________________________________

4) KCl _______________________________________________________

5) FeCl2 ______________________________________________________

6) FeCl3 ______________________________________________________

7) Zn(OH)2 ___________________________________________________

8) Be2SO4 ___________________________________________________

9) CrF2 ______________________________________________________

10) Al2S3 _____________________________________________________

11) PbO ______________________________________________________

12) Li3PO4 ____________________________________________________

13) TiI4 _______________________________________________________

14) Co3N2 ____________________________________________________

15) Mg3P2 ____________________________________________________

16) Ga(NO2)3 __________________________________________________

17) Ag2SO3 ____________________________________________________

18) NH4OH ____________________________________________________

19) Al(CN)3 ____________________________________________________

20) Be(CH3COO)2 ______________________________________________

#5


For the following compounds, give the formulas and the molar masses:

Formula Molar Mass

22) sodium phosphide ___________________________________________

23) magnesium nitrate ___________________________________________

24) lead (II) sulfite ______________________________________________

25) calcium phosphate ___________________________________________

26) ammonium sulfate ___________________________________________

27) silver cyanide _______________________________________________

28) aluminum sulfide ____________________________________________

29) beryllium chloride ____________________________________________

30) copper (I) arsenide ___________________________________________

31) iron (III) oxide _______________________________________________

32) gallium nitride _______________________________________________

33) iron (II) bromide _____________________________________________

34) vanadium (V) phosphate ______________________________________

35) calcium oxide _______________________________________________

36) magnesium acetate __________________________________________

37) aluminum sulfate ____________________________________________

38) copper (I) carbonate __________________________________________

39) barium oxide ________________________________________________

40) ammonium sulfite ____________________________________________

41) silver bromide _______________________________________________

42) lead (IV) nitrite ______________________________________________

Ionic Compound Naming – Chilton Honors Chemistry

Ionic Compound Formula Writing Worksheet Write chemical formulas for the compounds in each box. The names are found by finding the intersection between the cations and anions. Example: The first box is the intersection between the “zinc” cation and the “chloride” anion, so you should write “ZnCl2”, as shown.

zinc iron (II) iron (III) gallium silver lead (IV) chloride ZnCl2 acetate nitrate Oxide nitride sulfate

Write the formulas for the following compounds: 1) copper (II) chloride ____________________________________ 2) lithium acetate ____________________________________ 3) vanadium (III) selenide ____________________________________ 4) manganese (IV) nitride ____________________________________ 5) beryllium oxide ____________________________________ 6) sodium sulfate ____________________________________ 7) aluminum arsenide ____________________________________ 8) potassium permanganate ____________________________________ 9) chromium (VI) cyanide ____________________________________ 10) tin (II) sulfite ____________________________________ 11) vanadium (V) fluoride ____________________________________ 12) ammonium nitrate ____________________________________

#6

Ionic Compound Naming – Chilton Honors Chemistry

Names & Formulas for Ionic Compounds Give the name or formula of the following ionic compounds:

Name 1) Na2CO3 ____________________ 2) NaOH ______________________ 3) MgBr2 ______________________ 4) KCl ________________________ 5) FeCl2 _______________________ 6) FeCl3 _______________________ 7) Zn(OH)2 _____________________ 8) Be2SO4 _____________________ 9) CrF2 ________________________ 10) Al2S3 _______________________ 11) PbO ________________________

12) Li3PO4 ______________________ 13) TiI4 _________________________ 14) Co3N2 ______________________ 15) Mg3P2 ______________________ 16) Ga(NO2)3 ____________________ 17) Ag2SO3 ______________________ 18) NH4OH ______________________ 19) Al(CN)3 ____________________ 20) Be(CH3COO)2 ________________

Formula 21) sodium phosphide _____________ 22) magnesium nitrate _____________ 23) lead (II) sulfite _________________ 24) calcium phosphate _____________ 25) ammonium sulfate _____________ 26) silver cyanide _________________ 27) aluminum sulfide ______________ 28) beryllium chloride ______________ 29) copper (I) arsenide _____________ 30) iron (III) oxide _________________ 31) gallium nitride _________________ 32) iron (II) bromide _______________ 33) vanadium (V) phosphate ________ 34) calcium oxide _________________ 35) magnesium acetate ____________ 36) aluminum sulfate ______________ 37) copper (I) carbonate ____________ 38) barium oxide __________________ 39) ammonium sulfite ______________ 40) silver bromide _________________

#6b


Balancing Chemical Equations

Balance the equations below:

1) ____ N2 + ____ H2 Æ ____ NH3

2) ____ KClO3 Æ ____ KCl + ____ O2

3) ____ NaCl + ____ F2 Æ ____ NaF + ____ Cl2

4) ____ H2 + ____ O2 Æ ____ H2O

5) ____ Pb(OH)2 + ____ HCl Æ ____ H2O + ____ PbCl2

6) ____ AlBr3 + ____ K2SO4 Æ ____ KBr + ____ Al2(SO4)3

7) ____ CH4 + ____ O2 Æ ____ CO2 + ____ H2O

8) ____ C3H8 + ____ O2 Æ ____ CO2 + ____ H2O

9) ____ C8H18 + ____ O2 Æ ____ CO2 + ____ H2O

10) ____ FeCl3 + ____ NaOH Æ ____ Fe(OH)3 + ____NaCl

11) ____ P + ____O2 Æ ____P2O5

12) ____ Na + ____ H2O Æ ____ NaOH + ____H2

13) ____ Ag2O Æ ____ Ag + ____O2

14) ____ S8 + ____O2 Æ ____ SO3

15) ____ CO2 + ____ H2O Æ ____ C6H12O6 + ____O2

16) ____ K + ____ MgBr Æ ____ KBr + ____ Mg

17) ____ HCl + ____ CaCO3 Æ ____ CaCl2 + ____H2O + ____ CO2

18) ____ HNO3 + ____ NaHCO3 Æ ____ NaNO3 + ____ H2O + ____ CO2

19) ____ H2O + ____ O2 Æ ____ H2O2

20) ____ NaBr + ____ CaF2 Æ ____ NaF + ____ CaBr2

21) ____ H2SO4 + ____ NaNO2 Æ ____ HNO2 + ____ Na2SO4

#7

Writing'Chemical'Equations''Part%A'–'Translate)all)the)formulaic)equations)to)word)equations.))'

'

1. Na2O'+'H2O''NaOH'2. 2HgO(s)''2Hg(l)'+'O2(g)'3. BaCl2(aq)'+'Na2CrO4(aq)''BaCrO4(s)'+'2NaCl(aq)'4. CS2(l)'+'3O2(g)''CO2(g)'+'2SO2(g)'5. NaCl(aq)'+'AgNO3(aq)''NaNO3(aq)'+'AgCl(s)'6. H2(g)'+'Cl2(g)''2HCl(g)'7. 2H2O(l)''2H2(g)'+'O2(g)'8. Zn(s)'+'HCl(aq)''ZnCl2(aq)'+'H2(g)'9. Al4C3(s)'+'H2O(l)''CH4(g)'+'Al(OH)3(s)'10. Al2(SO4)3'+'Ca(OH)2''Al(OH)3'+'CaSO4'11. 2K(s)'+'2H2O(l)''2KOH(aq)'+'H2(g)'12. H2SO4(aq)''SO3(g)'+'H2O(l)'13. 2KClO3(s)''2KCl(s)'+'3O2(g)'14. CH3OH(g)'+'O2(g)''CO2(g)'+'H2O(g)''Part%B'–'Translate)all)the)word)equations)to)formulaic)equations)and)then)balance)them.'

'

1. Sodium'combines'with'chlorine'to'produce'sodium'chloride.'2. When'solid'copper'reacts'with'aqueous'silver'nitrate,'the'products'are'aqueous'copper'II'

nitrate'and'silver'metal.'3. Solid'iron'III'oxide'and'carbon'monoxide'gas'produce'iron'metal'and'carbon'dioxide'gas.'4. Sulfuric'acid'and'sodium'hydroxide'react'to'form'sodium'sulfate'and'water.'5. Vanadium'II'oxide'with'iron'III'oxide'results'in'the'formation'of'vanadium'V'oxide'and'iron'II'

oxide.'6. Aluminum'reacts'with'oxygen'to'produce'aluminum'oxide.'7. Mercury'II'oxide'decomposes'to'produce'mercury'and'oxygen'8. Sodium'carbonate'decomposes'to'produce'sodium'oxide'and'carbon'dioxide'9. Carbon'dioxide'gas'reacts'with'solid'lithium'hydroxide'to'produce'solid'lithium'carbonate'and'

water.'10. Ammonia'gas'reacts'with'oxygen'gas'to'produce'nitrogen'monoxide'gas'and'steam.'11. Solid'ammonium'nitrate'decomposes'to'produce'dinitrogen'monoxide'gas'and'water.'12. Carbon'monoxide'reacts'with'hydrogen'to'produce'methanol.'13. Liquid'carbon'disulfide'reacts'with'oxygen'gas'to'produce'carbon'dioxide'gas'and'sulfur'

dioxide'gas.'14. Aluminum'metal'reacts'with'aqueous'copper'II'chloride'to'produce'aqueous'aluminum'

chloride'and'solid'copper.'15. Solid'ammonium'chloride'decomposes'to'produce'ammonia'gas'and'gaseous'hydrochloric'

acid.''

#8


Predicting Reaction Products

Balance the equations and predict the products for the following reactions:

1) ____ Na + ____ FeBr3 Æ

2) ____ NaOH + ____ H2SO4 Æ

3) ____ C2H4O2 + ____ O2 Æ

4) ____ NH3 + ____ H2O Æ

5) ____ PbSO4 + ____ AgNO3 Æ

6) ____ PBr3 Æ

7) ____ HBr + ____ Fe Æ

8) ____ KMnO4 + ____ ZnCl2 Æ

9) ____MnO2 + ____ Sn(OH)4 Æ

10) ____ O2 + ____ C5H12O2 Æ

11) ____ H2O2 Æ

12) ____ PtCl4 + ____ Cl2 Æ

#9

StoichiometryWorksheet

1.Na2SIO3(s)+8HF(aq)H2SiF6(aq)+2NaF(aq)+3H2O(l)

a.HowmanymolesofHFareneededtoreactwith0.300molofNa2SiO3?

b.HowmanygramsofNaFformwhen0.500molofHFreactswithexcessNa2SiO3?

c.HowmanygramsofNa2SiO3canreactwith0.800gofHF?

2.C6H12O6(aq)2C2H5OH(aq)+2CO2(g)

a.HowmanymolesofCO2areproducedwhen0.400molofC6H12O6reactsinthis

fashion?

b.HowmanygramsofC6H12O6areneededtoform7.50gofC2H5OH?

c.HowmanygramsofCO2formwhen7.50gofC2H5OHareproduced?

3.Fe2O3(s)+CO(g)Fe(s)+CO2(g)(unbalanced!)

a.CalculatethenumberofgramsofCOthatcanreactwith0.150kgofFe2O3

#10

b.CalculatethenumberofgramsofFeandthenumberofgramsofCO2formed

when0.150kgofFe2O3reacts

4.2NaOH(s)+CO2(g)Na2CO3(s)+H2O(l)

a.Whichreagentisthelimitingreactantwhen1.85molNaOHand1.00molCO2are

allowedtoreact?

b.HowmanymolesofNa2CO3canbeproduced?

5.C6H6+Br2C6H5Br+HBr

a.WhatisthetheoreticalyieldofC6H5Brinthisreactionwhen30.0gofC6H6reacts

with65.0gorBr2?

b.IftheactualyieldofC6H5Brwas56.7g,whatisthepercentyield?

Stoichiometry: Mass-Mass Problems

1. 2KClO3 → 2KCl + 3O2

How many grams of potassium chloride, KCl, are produced if 25.0g of potassium chlorate, KClO3, decompose? 2. N2 + 3H2 → 2NH3 How many grams of hydrogen, H2, are necessary to react completely with 50.0 g of nitrogen, N2?

3. How many grams of ammonia, NH3, are produced in the reaction with 50.0 g of N2, nitrogen, in Problem 2? 4. 2AgNO3 + BaCl2 → 2AgCl + Ba(NO3) 2 How many grams of AgCl, silver chloride, are produced from 5.0 g of AgNO3, silver nitrate?

5. How many grams of BaCl2, barium chloride, is necessary to react with the 7.5 g AgNO3, silver nitrate, in Problem 4?

#11


Percent, Actual, and Theoretical Yield1) LiOH + KCl Æ LiCl + KOH

a) I began this reaction with 20 grams of lithium hydroxide. What is mytheoretical yield of lithium chloride?

b) I actually produced 6 grams of lithium chloride. What is my percentyield?

2) C3H8 + 5 O2 Æ 3 CO2 + 4 H2O

a) If I start with 5 grams of C3H8, what is my theoretical yield of water?

b) I got a percent yield of 75% How many grams of water did I make?

3) Be + 2 HCl Æ BeCl2 + H2

My theoretical yield of beryllium chloride was 10.7 grams. If my actualyield was 4.5 grams, what was my percent yield?

4) 2 NaCl + CaO Æ CaCl2 + Na2O

What is my theoretical yield of sodium oxide if I start with 20 grams ofcalcium oxide?

#12


5) FeBr2 + 2 KCl Æ FeCl2 + 2 KBr

a) What is my theoretical yield of iron (II) chloride if I start with 34 gramsof iron (II) bromide?

b) What is my percent yield of iron (II) chloride if my actual yield is 4grams?

6) TiS + H2O Æ H2S + TiO

What is my percent yield of titanium (II) oxide if I start with 20 grams oftitanium (II) sulfide and my actual yield of titanium (II) oxide is 22 grams?

7) U + 3 Br2 Æ UBr6

What is my actual yield of uranium hexabromide if I start with 100 gramsof uranium and get a percent yield of 83% ?

8) H2SO4 Æ H2O + SO3

If I start with 89 grams of sulfuric acid and produce 7.1 grams of water,what is my percent yield?

Name: Per: Date: _________________Row

Thermochemistry Review Worksheet 1.Definitions: -Endothermic: -Exothermic: -Enthalpy: -Law of Conservation of Energy -Heat of Reaction: -Heat of Fusion -Specific Heat 2. Explain why water is used in a calorimeter? What unique properties does water have? Calculations:

1. How many Joules of heat energy would be required to raise the temperature of 16.0g of lead from 25˚C to its melting point of 327˚C for a length of time long enough to completely melt the lead. Given: The specific heat capacity of lead is 0.159J/gK and the molar enthalpy of fusion is 24.7J/g.

Specific heat is in Kelvin. Must convert C to Kelvin.

Q=mcΔT Q=1460J 2. How much energy is absorbed by 300g of methanol, CH3OH, as it evaporates?

Given: The molar heat of vaporization is 35.3kJ/mol.

300 * (1/45.02) * (35.3/1) = 200 J (1 sigfig)

3. If 540g of water condenses on a car during a cool night, calculate the amount of energy released to the air during this condensation. Given: The molar heat of vaporization of water is 40.79kJ/mol.

540 * (1/18.02) * (40.79/1) = 1200kj 2 sig figs

#13

4. Calculate the amount of energy that is needed to change 125g of ice at -25˚C to water at 75˚C. Be sure to sketch a Phase Diagram of this process before beginning the work. Given: Molar enthalpy of fusion is 6.009kJ/mol, molar enthalpy of vaporization is 40.79kJ/mol, the specific heat of solid H2O is 2.1J/gK, the specific heat of liquid H2O is 4.186J/gK, and the specific heat of gas H2O is 1.7J/gK.

125 * 2.1 * 100 = 26000kj

5. What is the molar enthalpy of the formation of 1mol H2SO4(l) given the following information?

2H2(g) + O2(g) ! 2H2O(g) ΔHrxn = -484kJ 2S(s) + 3O2(g) ! 2SO3(g) ΔHrxn = -890kJ H2(g) + 2O2(g) + S(s)! H2SO4(l) ΔHrxn = -814kJ H2O(g) + SO3(g)! H2SO4(l) ΔHrxn = xkJ 115KJ

6. What is the molar enthalpy of the formation of 1mol C2H6 gas given the following information?

C2H4(g) + 3O2(g) ! 2CO2(g) + 2H2O(l) ΔHrxn = -1401kJ 2C2H6(g) + 7O2(g) ! 4CO2(g) + 6H2O(l) ΔHrxn = -3100kJ 2H2(g) + O2(g) ! 2H2O(l) ΔHrxn = -572kJ C2H4(g) + H2(g)! C2H6(g) ΔHrxn = xkJ -137KJ

7. The reaction for the fermentation of glucose is … C6H12O6 (aq) ! 2CO2(g) + 2C2H5OH(aq) ΔHrxn = -67kJ

a. Is this reaction endothermic or exothermic? b. Calculate the energy released when 250g of glucose C6H12O6 (aq) ferments.

250 * (1/180.07) * (-67/1) = -93KJ

Documents

AP#Chemistry#Summer#Work# - 2018 Mr.#Herring# · scientific notation worksheet #1 name_____ express each of the following numbers in proper scientific notation: