FINAL EXAM REVIEW PROBLEMS
Equations – These will be given to you on the exam
Acids and Bases
[H+][OH-] = 1.0 x 10-14 = Kw
pOH = -log [OH-]
pH + pOH = 14.00
[H+] = 10-pH
pH = -log [H+]
[OH-] = 10-pOH
Gas Laws
PV = nRT R = 0.0821 L atm/mol K V1 /T1 = V2 /T2
V1 /n1 = V2 /n2
P1V1/T1 = P2V2 /T2
P1V1 = P2V2
Ptotal = P1 + P2 + …
Solutions
Molarity = moles
liters
density = __m__
V
M1V1 = M2V2
Energy
q = mcΔT
moles =
mass
molar mass
MacidVacid = MbaseVbase
1.00 cal = 4.184 J
Equilibrium
K = [Products]/[Reactants]
Basics
1. Write the numbers 4300 and 0.0102 in scientific notation.
2. Give the number of significant figures for each of the following:
a. 0.00100
b. 2.0800 x 102
c. 480
3. Give the answer for each calculation to the correct number of significant figures:
a. 12.6 X 0.53
b. (25.36 –4.15)  2.317
c. (2.6 x .42) – 4.59
4. Which temperature is colder, 172 K or -75C? _________________
5. An antifreeze solution in a car’s radiator boils at 239F. What is the temperature on
the Celsius scale?
a.
22oC
b.
-16 oC
c. 115 oC
d. 458 oC
6. Write the formula for each of the following compounds, list the elements in order
given:
a. A molecule contains four phosphorus atoms and ten oxygen atoms _____
b. A molecule contains one sulfur atom and six fluorine atoms
_____
c. A molecule contains one aluminum atom and three chlorine atoms _____
7. Write the formula for each of the following compounds.
a. ammonium sulfate
g. aluminum oxide
b. vanadium (V) fluoride
h. lead (IV) oxide
c. disulfur dichloride
i. cobalt (III) nitrate
d. rubidium peroxide
j. calcium chloride
e. nitrous acid
k. hydroiodic acid
f. bromic acid
l. phosphoric acid
8. Name the following compounds.
a. Rb2O
b. K2S
c. PbBr4
d. Fe2S3
e. SrI2
f. KMnO4
g. Zn3(PO4)2
h. CsClO3
i. CuCl
j. NaHCO3
k. (NH4)2Cr2O7
l. FeS
m. PbBr2
n. Cu(NO3)2
o. NF3
p. SF2
q. CCl4
r. HF
s. HCl
t. HC2H3O2
u. HNO3
v. H2SO3
9. Calculate the number of moles and the mass of a sample of chromium containing
5.00 x 1018 atoms.
10.
Calculate the molar mass of HC2H3O2.
11.
Explain what Avogadro’s number represents?
12.
A 314.5 g Na2SO3 represents how many moles?
13.
Calculate the mass percent of each element in C14H20N2SO4.
14. In an experiment it was observed that 0.6884 g of lead combines with 0.2356 g of
chlorine to form a binary compound. Calculate the empirical formula of this
compound.
15. A gasoline additive is 71.65% Cl, 24.27% C, and 4.07% H. The molar mass is
98.96 g. Determine the empirical formula and the molecular formula.
Stoichiometry
C3H8
+ 5 O2  3 CO2 + 4 H2O
16. Calculate the moles of CO2 formed when 4.30 mol of C3H8 reacts with the
required 21.5 mol of O2.
17. What mass of carbon dioxide is produced when 82.6 g of C3H8 reacts with
sufficient oxygen?
6 Li(s) + N2 (g)  2 Li3N (s)
18. Calculate the mass of lithium nitride formed from 56.0 g of nitrogen gas and 56.0
g of lithium:
TiCl4 (g) + O2 (g)  TiO2 (s) + 2 Cl2 (g)
19. Suppose 6.71 x 103 g of titanium (IV) chloride is reacted with 2.45 x 103 g of
oxygen.
a. Calculate the maximum mass of titanium (IV) oxide that can form.
b. If the percent yield of TiO2 is 75%, what mass was actually produced?
Gas Laws
20. What volume does 1 mole of gas occupy at STP?
21. A sample of neon to be used in a neon sign has a volume of 1.51 L at a pressure
of 615 torr. Calculate the volume of the gas after it is pumped into the glass tubes
of the sign, where it shows a pressure of 795 torr.
22. A child blows a bubble that contains air at 28C and has a volume of 23 mL at 1
atm. As the bubble rises, it encounters a pocket of cold air. If there is no change
in pressure, will the bubble get larger or smaller as the air inside cools to 18C?
Calculate the new volume.
23. Consider two sample of nitrogen gas. Sample 1 contains 1.5 mol of N2 and has a
volume of 36.7 L at 25C and 1 atm. Sample 2 has a volume of 16.5 L at 25C
and 1 atm. Calculate the number of moles of N2 in sample 2.
24. A weather balloon contains 1.10 x 103 mol of helium and has a volume of 2.70 x
104 L at 1.00 atm of pressure. Calculate the temperature of the helium in the
balloon in Kelvin and in degrees Celsius.
25. A 2.0 L flask contains a mixture of nitrogen gas and oxygen gas at 25C. The
total pressure of the gaseous mixture is 0.91 atm and the mixture is known to
contain 0.050 mol of N2. Calculate the partial pressure of oxygen and moles of
oxygen present.
Zn + 2 HCl  ZnCl2 + H2
26. Calculate the volume of hydrogen produced at STP by the reaction by the reaction
of 24.3 g of zinc with excess HCl according to the equation above.
27. A sample of NH3 occupies 5.00 L at 23C and 13.5 atm. What volume will the
sample occupy at STP?
Solutions
28. A student wants to identify the main component in a commercial liquid cleaner.
He finds that 35.8 mL of the cleaner weighs 28.1 g. Of the following
possibilities, which is the main component of the cleaner?
chloroform
1.483 g/mL
diethyl ether
0.714 g/mL
isopropyl alcohol
0.785 g/mL
toluene
0.867 g/mL
29. What is the difference between a saturated and unsaturated solution?
30. What is the difference between a concentrated and dilute solution?
31. How can you create a supersaturated solution?
32. A 126 g sample of seawater is evaporated to dryness, leaving 4.73 g of solid
residue. Calculate the mass percent of solute present in the original seawater.
33. What mass of water must be added to 425 g of formaldehyde to prepare a 40.0%
solution of formaldehyde?
34. Calculate the molarity of a solution prepared by dissolving 2.75 g of ethanol,
C2H5OH, in enough water to give a final volume of 101 mL.
35. Give the concentrations of the ions in each of the following solutions assuming all
of the solid dissolves:
a. 0.10 M Na2CO3
b. 0.010 M Al2(SO4)3
36. Calculate the number of moles of Cl- ions in 1.75 L of 1.0 x 10-3 M AlCl3.
37. What volume of 12 M HCl must be used to prepare 0.75 L of 0.45 M HCl?
38. Calculate the exact volume of 0.10 M HNO3 needed to completely neutralize
125.0 mL of 0.50 M KOH.
39. What volume of 0.50 M H2SO4 is required to react exactly with 0.250 L of 0.80
M KOH?
Energy, Solids, and Liquids
40. How many calories of energy correspond to 33.6 J?
41. Perform the indicated conversions.
c. 45.62 kcal to kJ
d. 2.751 kJ to cal
c. 72.94 kJ to kcal
d. 5.721 kcal to J
42. Calculate the joules of energy required to heat 298 g of water (c = 4.18 J/goC)
from 7.6C to 81.5C?
43. A 5.63 g sample of metal is heated from 21C to 32C. This change in
temperature requires 8.05 J of energy. What is the specific heat capacity of this
metal?
44. For question below determine if the molecule would be polar or nonpolar. Would
it have hydrogen bonding, dipole – dipole, or London dispersion forces?
e. NF3
c. SF2
f. HF
d. CCl4
45. If the system is defined as the underlined item, are the following processes
exothermic or endothermic?
g. When solid KBr is dissolved in water, the solution gets colder.
h. CH4 is burned in a furnace.
i. When concentrated sulfuric acid is added to water it gets very hot.
j. Water is warmed in a tea kettle.
46. Draw the heating and cooling curve for water and label it.
47. Draw the phase diagram for water and label it.
Acids and Bases
48. Which of the following represent conjugate acid-base pairs?
a. H2O,H3O+
b. OH-,HNO3
c. H2SO4,SO4-2
d. HC2H3O2,C2H3O249. Calculate the [H+] in a solution in which [OH-] = 2.0 x 10-2M. Is this solution
acidic, neutral, or basic?
50. Calculate the pH value for each of the following solutions at 25C:
a. A solution in which [H+] = 1. x 10-3 M
b. A solution in which [OH-] = 5.0 x 10-5 M
51. A sample of rain in an area with severe air pollution has a pH of 3.5. What is the
pOH of this rainwater?
52. The pOH of a liquid drain cleaner was found to be 10.50. What is the [OH-] for
this cleaner?
53. The pH of rainwater in a polluted area was found to be 5.75. What is the [H+]?
54. Calculate the pH of a solution of 5.0 x 10-3 M HCl.
Chemical Equilibrium and Kinetics
55.
Write the equilibrium expression for each of the following reactions:
a. 4 NH3 (g) + 7 O2 (g)  4 NO2 (g) + 6 H2O (g)
b. S(s) + O2 (g)  SO2 (g)
c. P4 (g) + 6 Cl2 (g)  4 PCl3 (g)
d. 2 AlCl3 (s)  2 Al (s) + 3 Cl2 (g)
e. Suggest a method for shifting these reactions toward the products.
56.
For each of the following reactions, predict the direction the equilibrium will shift
when the volume of the container is increased.
a. H2 (g) + F2 (g)  2 HF (g)
b. CO (g) + 2 H2 (g)  CH3OH (g)
c. 2 SO3 (g)  2 SO2 (g) + O2 (g)
57. For the reaction:
2 SO2 (g) + O2 (g)  2 SO3 (g)
a. If the reaction is exothermic would it give off or take in heat?
b.SO2 is added, which way would it shift?
c. SO3 is removed, which way would it shift?
d.The volume is decreased, which way would it shift?
e. The temperature is decreased, which way would it shift?
f. If the [SO2] = 4.5 x 10-2 , [O2] = 1.2 x 10-2 , and K = 1.00, then what is
[SO3] = ?
58. Write the balanced equation for the reaction describing the dissolving of each of
the following solids in water. Also write the Ksp expression for each solid.
a. BaSO4
b. Fe(OH)2
c. Ag2SO4
59. Calculate the Ksp value for barium sulfate has a solubility of 3.9 x 10-5 M at 25C.
60. The Ksp value for PbCrO4 is 2.0 x 10-16 at 25C. Calculate the solubility.