1. AP Chemistry – 1st Semester Final Exam Review Chapters 1 – 9
1. Ch3 #73. Benzene contains only carbon and hydrogen and is 7.74% H by mass; the molar mass of benzene is 78.1 g/mol.
Determine the empirical and molecular formulas of benzene.
Assume 100 g sample:

2. Molecular Formula Mass Empirical Formula Mass
1. Ch3 #73. Benzene contains only carbon and hydrogen and is 7.74% H by mass; the molar mass of benzene is 78.1 g/mol.
Determine the empirical and molecular formulas of benzene.
Assume 100 g sample:
1:1
Empirical Formula: CH
Molecular Formula Mass
Empirical Formula Mass

3. b. Iron (III) sulfide reacts with gaseous hydrogen chloride …
Ch3 #80) Balanced chem reactions:
a. Glucose (C6H12O6) reacts w oxygen…
b. Iron (III) sulfide reacts with gaseous hydrogen chloride …

4. Ch3 #100. Mercury and Bromine will react with each other to produce
mercury (II) bromide
Hg(l) + Br2(l) HgBr2(s)
10.0 g g
a. What mass of HgBr2 can be produced from the reaction of 10.0 g Hg
and 9.00 g Br2? What mass of which reagent is left unreacted?
Hg is L.R.

5. Ch3 #100. Mercury and Bromine will react with each other to produce
mercury (II) bromide
Hg(l) + Br2(l) HgBr2(s)
10.0 g g
a. What mass of HgBr2 can be produced from the reaction of 10.0 g Hg
and 9.00 g Br2? What mass of which reagent is left unreacted?
Hg is L.R.

6. 100. Mercury and Bromine will react with each other to produce
mercury(2) bromide
Hg(l) + Br2(l) HgBr2(s)
5ml ml
b. What mass of HgBr2 can be produced from the reaction of
5.00 mL mercury (density = g/ml) and
5.00 mL bromine (density = 3.10 g/ml)?

7. Ch4 #15.Calculate the molarity of each of these solutions.
a. A 5.623g sample of NaHCO3 is dissolved in enough water
to make 250 ml of solution.

8. Ch4 #15.Calculate the molarity of each of these solutions.
a. A 5.623g sample of NaHCO3 is dissolved in enough water
to make 250 ml of solution.

9. Ch4 #23. Describe how you would prepare 2
Ch4 #23. Describe how you would prepare 2.00 L of each of the following
solutions.
a M NaOH from solid NaOH
b M NaOH from 1.00M NaOH stock solution
b M1.V1 = M2.V2

10. Ch4 #43. A 100.0mL aliquot of 0.200 M aqueous potassium hydroxide is mixed
with mL of M aqueous magnesium nitrate.
a. Write a balanced chemical equation for any reaction that occurs.
b. What mass of precipitate is produced?
c. Calculate the concentration of each ion remaining in solution after precipitation is complete.

11. 2KOH + Mg(NO3)2  2K+ + 2NO3- + Mg2+ + 2OH-
Ch4 #43. A 100.0mL aliquot of M aqueous potassium hydroxide is mixed
with mL of M aqueous magnesium nitrate.
a. Write a balanced chemical equation for any reaction that occurs.
b. What mass of precipitate is produced?
c. Calculate the concentration of each ion remaining in solution after precipitation is complete.
2KOH + Mg(NO3)2  2K+ + 2NO Mg OH-
2KOH + Mg(NO3)2  Mg(OH)2(s)
0.200M M
100ml ml

12. a. KMnO4 b. NiO2 e. P4O6 f. Fe3O4 h. SF4 i. CO Ch4
57. Assign oxidation states for all atoms in each of the following compounds.
a. KMnO4 b. NiO2
e. P4O6 f. Fe3O4
h. SF4 i. CO

13. a. KMnO4 b. NiO2 e. P4O6 f. Fe3O4 h. SF4 i. CO Ch4
57. Assign oxidation states for all atoms in each of the following compounds.
a. KMnO4 b. NiO2
(+1)+7(-8) (-4)
e. P4O6 f. Fe3O4
h. SF4 i. CO

14. Ch4
65. Balance the following oxidation-reductions reactions that occur in basic solutions.
a. Al(s) + MnO4-(aq) MnO2(s) + Al(OH)4-(aq)

15. Ch4
62a. Specify if Cu(s) + 2Ag+(aq)  2Ag(s) +Cu2+(aq) is a oxidation-reduction reaction, and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced.

16. Ch5
30. A balloon is filled to a volume of 7.00x102 mL at a temperature
of 20.0°C. The balloon is then cooled at a constant pressure to a temperature of 1.00x102 K. What is the final volume of the balloon?
V1 = .700L V2 = ?
P1 = const P2 = const
T1 = 293K T2 = 100.K
V2 =

17. Ch5
38. What volume is occupied by 2.0 g of He at 25˚C and a pressure
of 775 mm Hg?
P.V = n.R.T

18. Ch5
38. What volume is occupied by 2.0 g of He at 25˚C and a pressure
of 775 mm Hg?
P.V = n.R.T

19. Ch5
49. Calculate the volume of O2, at STP, required for the complete combustion of 125 g octane (C8H18) to CO2 and H2O.
2C8H O2  16CO H2O
125g ?L

20. 55. Hydrogen cyanide is prepared commercially by the reaction of methane, CH4(g), ammonia, NH3(g), and oxygen, O2(g), at high temperature. The other product is gaseous water.
a. Write a chemical equation for the reaction.
CH4 + NH3 + O2 
b. What volume of HCN(g) can be obtained from 20 L CH4(g),
20 L NH3(g), and 20 L O2(g)? The volumes are all measured
at the same temperature and pressure.

21. 2CH4 +2NH3 +3O2 2HCN + 6H2O
20L 20L 20L ?L
At same temp and pressure, equal volumes contain equal number moles.
(Assume STP, vol conv cancels out.)
b. What volume of HCN(g) can be obtained from 20 L CH4(g),
20 L NH3(g), and 20 L O2(g)? The volumes are all measured
at the same temperature and pressure.

22. 57. A gas consisting of only carbon and hydrogen has an empirical formula of CH2. The gas has a density of 1.65 g/L at 27oC and 734 torr. Determine the molar mass and molecular formula of the gas.
empirical formula: CH2  14.0 g/mol
molecular formula: CXH2X
d=1.65g/L
T=300K
P=734torr0.966atm

23. 57. A gas consisting of only carbon and hydrogen has an empirical formula of CH2. The gas has a density of 1.65 g/L at 27oC and 734 torr. Determine the molar mass and molecular formula of the gas.
empirical formula: CH2  14.0 g/mol
molecular formula: CXH2X
d=1.65g/L
T=300K
P=734torr0.966atm

24. 63. Consider the flasks diagrammed below, what are the partial pressures of H2 and N2 after the stopcock between the two flasks is opened? (Assume the final volume is 3 L) What is the final pressure in torr?
1.00 L N2
0.200 atm
2.00 L H2
475 torr

25. P1.V1 = P2.V2 (152torr)(1.00L) = P2.(3.00L) P1.V1 = P2.V2
63.
1.00 L N2
0.200 atm
(152torr)
P1.V1 = P2.V2
(152torr)(1.00L) = P2.(3.00L)
PN2 = 50.7torr (per 3L)
2.00 L H2
475 torr
P1.V1 = P2.V2
(475torr)(2.00L) = P2.(3.00L)
PH2 = 317torr (per 3L)
Ptotal =

26. 65. The partial pressure of CH4(g) is 0.175 atm and that of O2(g)
is atm in a mixture of the two gasses.
a. What is the mole fraction of each gas in the mixture?
b. If the mixture occupies a volume of 10.5 L at 65o C, calculate the total number of moles of gas in the mixture
c. Calculate the number of grams of each gas in the mixture.

27. 65. The partial pressure of CH4(g) is 0.175 atm and that of O2(g)
is atm in a mixture of the two gasses.
a. What is the mole fraction of each gas in the mixture?
b. If the mixture occupies a volume of 10.5 L at 65o C, calculate the total number of moles of gas in the mixture
Total =
c. Calculate the number of grams of each gas in the mixture.

28. 79. Consider three identical flasks filled with different gases.
Flask A: CO at 760 torr and 0oC m = 26.0 g/mol
Flask B: N2 at 250 torr and 0oC m = 28.0 g/mol
Flask C: H2 at 100 torr and 0oC m = 2.0 g/mol
a. in which flask will the molecules have the greatest average kinetic energy? KEave = ½m.(uave)2
b. In which flask will the molecules have the greatest average velocity?

29. 81. The effusion rate of an unknown gas is measured and found to be
31.50mL/min. Under identical experiment conditions,
the effusion rate of O2 is found to be 30.50mL/min.
If the choices are CH4, CO,NO,CO2, and NO2 what is the identity
of the unknown gas?
O2 : 32.0g/mol CH4 : 16.0g/mol
CO : 28.0g/mol
NO : 30.0g/mol
CO2 : 44.0g/mol
NO2 : 46.0g/mol

30. Ch6 #26. Consider the mixture of air and gasoline vapor in a cylinder with
a piston. The original volume is 40. cm3. If the combustion of this
mixture releases 950. J of energy, to what volume will the gases
expand against a constant pressure of 650. torr if all the energy of
combustion is conserved into work to push back the piston.

31. Ch6 #26. Consider the mixture of air and gasoline vapor in a cylinder with
a piston. The original volume is 40. cm3. If the combustion of this
mixture releases 950. J of energy, to what volume will the gases
expand against a constant pressure of 650. torr if all the energy of
combustion is conserved into work to push back the piston.
ΔV = (V2 – 0.040L)
q  W = –950J (expands – gas doing work)
W = –P. ΔV
–950J = –(86.6kPa). ΔV ΔV = 10.97L
10.97L = (V2 – 0.040L)

32. 29. The equation for the fermentation of glucose to alcohol
and carbon dioxide is
C6H12O6(aq) → 2C2H5OH(aq) + 2CO2(g)
The enthalpy change for the reaction is -67kJ.
Is the reaction exothermic or endothermic?
Is energy, in the form of heat, absorbed or evolved as the reaction occurs?

33. 34. The overall reaction in commercial heat packs can be represented
as 4Fe(s) + 3O2(g) → 2Fe2O3(s) ΔH = -1652kJ
c. How much heat is released when 1.00 g iron is reacted with
excess O2?
d. How much heat is released when 10.0 g Fe and 2.00 g O2
are reacted?

34. 34. The overall reaction in commercial heat packs can be represented
as 4Fe(s) + 3O2(g) → 2Fe2O3(s) ΔH = -1652kJ
c. How much heat is released when 1.00 g iron is reacted with
excess O2?
d. How much heat is released when 10.0 g Fe and 2.00 g O2
are reacted?
released

35. m=11g m=125g 47.Consider the dissolution of CaCl2:
CaCl2(s) → Ca2+(aq) + 2Cl-(aq) ΔH = kJ
An 11.0g sample of CaCl2 is dissolved in 125 g of water, with both substances at 25.0˚C. Calculate the final temperature of the solution assuming no heat lost to the surroundings and assuming the solution has a specific heat capacity of 4.18 J/˚C·g
CaCl2(s) water Ca2+(aq) + 2Cl-(aq) kJ
m=11g m=125g
Ti = 25C Ti = 25C per 1 mol CaCl2

36. m=11g m=125g 47. CaCl2(s) water Ca2+(aq) + 2Cl-(aq) + 81.5 kJ
Ti = 25C Ti = 25C per 1 mol CaCl2
q = – m.cp.ΔT

37. NO(g) + O3(g) → NO2(g) + O2(g) ΔH = -199 kJ
55. Given the following data:
2O3(g) → 3O2(g) ΔH = -427 kJ
O2(g) → 2O(g) ΔH = +495 kJ
NO(g) + O3(g) → NO2(g) + O2(g) ΔH = -199 kJ
calculate ΔH for the reaction

38. NO(g) + O3(g) → NO2(g) + O2(g) ΔH = -199 kJ
55. Given the following data:
2O3(g) → 3O2(g) ΔH = -427 kJ
O2(g) → 2O(g) ΔH = +495 kJ
NO(g) + O3(g) → NO2(g) + O2(g) ΔH = -199 kJ
calculate ΔH for the reaction
2NO(g) + 2O3(g) → 2NO2(g) +2O2(g) ΔH = -398 kJ
3O2(g) → 2O3(g) ΔH = +427 kJ
2O(g) → O2(g) ΔH = -495 kJ
2NO(g) + 2O(g) → 2NO2(g) ΔH = -466 kJ
NO(g) + O(g) → NO2(g) ΔH = -233 kJ

39. a. 2NH3(g) + 3O2(g) + 2CH4(g) → 2HCN(g) + 6H2O(g)
61. Use the values of ΔHfo in Appendix 4 to the calculate ΔHo for the following reactions.
a. 2NH3(g) + 3O2(g) + 2CH4(g) → 2HCN(g) + 6H2O(g)
2mol(-46kJ/mol)+ 3(0) + 2mol(-75kJ/mol) 2mol(135.1kJ/mol) + 6mol(-242kJ/mol)
ΔHoreaction =

40. 43. It takes 7.21 x J of energy to remove an electron from an iron atom. What is the maximum wavelength of light that can do this? IE
e-1
nucleus

41. 43. It takes 7.21 x J of energy to remove an electron from an iron atom. What is the maximum wavelength of light that can do this? IE
e-1
nucleus

42. 45. Calculate the de Broglie wavelength for each of the following.
a. a proton with a velocity 90.% of the speed of light

43. 45. Calculate the de Broglie wavelength for each of the following.
a. a proton with a velocity 90.% of the speed of light

44. 49. Calculate the wavelength of light emitted when each of the following transition occur in the hydrogen atom.
a. n=3 n=2
n=4
n=3
n=2
n=1

45. 49. Calculate the wavelength of light emitted when each of the following transition occur in the hydrogen atom.
n=4
n=3
n=2
n=1
a. n=3 n=2

46. 83. Arrange the following groups of atoms in order of increasing size.
a. Be, Mg, Ca
85. Arrange the atoms in order of increasing first ionization energy.

47. 87. In each of the following sets, which atom or ion has the smallest
87. In each of the following sets, which atom or ion has the smallest radius?
c. O+, O, O-
d. S, Cl, Kr

48. 121) The successive ionization energies for an unknown element are:
I1 = 896kJ/mol
I2 = 1752 kJ/mol
I3 = 14,807 kJ/mol
I4 = kJ/mol
To which family in the periodic table does the unknown element most
likely belong?

49. 122) An unknown element is a nonmetal and has a valence electron
122) An unknown element is a nonmetal and has a valence electron configuration of ns2np4
a) How many valence electrons does this element have?
b) What are some possible identities for this element?
c) What is the formula of the compound this element would form
with potassium?
d) Would this element have a larger or smaller radius than barium?
e) Would this element have a greater or smaller ionization energy
than fluorine?

50. Ch8
1. Explain the electronegativity trends across a row and down a column of the periodic table. Compare these trends with those of ionization energies and atomic radii. How are they related?

51. 21. Without using Fig. 8.3, predict which bond in each of the following
groups will be the most polar.
a. C---F, Si---F, Ge---F
most
b. P---Cl, S---Cl
c. S---F, S---Cl, S---Br
d. Ti---Cl, Si---Cl, Ge---Cl

52. 64. Lewis structures that obey octet rule for each
64. Lewis structures that obey octet rule for each. (1st atom is central atom.)
a. POCI3, SO42- , XeO4, PO43- , CIO4-