1. Semester 2 Final Review
College Chemistry

2. Solutions/Kinetics #1
How many grams of calcium chloride are needed to prepare 5.0 L of 0.25 M solution?

3. Solutions/Kinetics #2
Adding which of the following to 1.0 kg of water would result in a solution with the highest boiling temperature?
a) 1.5 mol RbCl
b) 1.0 mol CO2
c) 75 g RbCl
d) 75 g CsCl

4. Solutions/Kinetics #3
Trial
[A]
[B]
[C]
Rate (M/s) 1
0.1
0.05
1.85 x 10-5 2
0.2
0.15
5.55 x 10-5 3
1.11 x 10-4 4
Use the data above to determine the rate law for this reaction. Also calculate the value of the rate constant, k, and be sure to include the proper units.

5. (NH4)2Se (s) ↔ NH3 (g) + H2Se (g)
Equilibrium #1
Write the equilibrium expression for the reaction below.
(NH4)2Se (s) ↔ NH3 (g) + H2Se (g)

6. Equilibrium #2
Write the equilibrium expression for the equilibrium reaction where dinitrogen tetroxide forms nitrogen dioxide.

7. Equilibrium #3 Consider the following chemical reaction:
H2 (g) + I2 (g) ↔ 2HI (g)
At equilibrium in a particular experiment, the concentrations of H2 = 3.5 x 10-3 M, I2 = 6.8 x 10-3 M, and HI = 7.8 x 10-7 M. Determine the value of the equilibrium constant.

8. Equilibrium #4 The equilibrium constant for the following reaction
N2 (g) + 3H2 (g) ↔ 2NH3 (g)
is Keq = 4.34 x 10-3 at 300°C. Describe the relative amounts of the reactants and products.

9. 2CO2 (g) ↔ 2CO (g) + O2 (g) DH° = -514 kJ
Equilibrium #5
Consider the following reaction at equilibrium:
2CO2 (g) ↔ 2CO (g) + O2 (g) DH° = -514 kJ
What happens to the equilibrium when CO2 is added to the reaction vessel?
List three other things you could do to this system to shift the equilibrium to the right.

10. Equilibrium #6 The reaction below is exothermic:
2SO2 (g) + O2 (g) ↔ 2SO3 (g)
List three things you could do to increase the amount of SO3 (g) in the reaction container.

11. CaCO3 (s) ↔ CaO (s) + CO2 (g)
Equilibrium #7
For the endothermic reaction
CaCO3 (s) ↔ CaO (s) + CO2 (g)
List two things you could do to increase the amount of CO2 (g) in the reaction vessel.

12. Redox #1 What is the oxidation number of chromium in the Cr2O7-2 ion?
b. 2Cr3+

13. KMnO4 + HCl → MnCl2 + Cl2 + H2O + KCl
Redox #2
In the reaction below…
a. What element is reduced?
b. What element is oxidized?
KMnO4 + HCl → MnCl2 + Cl2 + H2O + KCl
2Cr3+
b. 2Cr3+

14. Redox #3 In the reaction below… a. What element is oxidized?
b. Write the oxidation half-reaction.
Cr2O S2O H+ → 2Cr S4O H2O Cr

15. Redox #4 Write the reduction half reaction for this reaction.
3MnO4- (aq) H+ (aq) + 5Fe (s) → 3Mn2+ (aq) + 5Fe3+ (aq) H2O (l)

16. Sn2+ (aq) + 2Fe3+ (aq) → 2Fe2+ (aq) + Sn4+ (aq)
Redox #5
Determine the cell potential for this reaction.
Sn2+ (aq) + 2Fe3+ (aq) → 2Fe2+ (aq) + Sn4+ (aq)
2Cr3+
b. 2Cr3+

17. Cr (s) + 3Fe3+ (aq) → 3Fe2+ (aq) + Cr3+ (aq)
Redox #6
Determine the standard electrical potential for this reaction.
Cr (s) + 3Fe3+ (aq) → 3Fe2+ (aq) + Cr3+ (aq)
2Cr3+
b. 2Cr3+

18. Pb2+ (aq) + Zn (s) → Zn2+ (aq) + Pb (s)
Redox #7
The standard cell potential (E°cell) for the reaction below is V. Calculate the cell potential if [Zn2+] = 1.0 M and [Pb2+] = 2.0 x 10–4 M.
Pb2+ (aq) + Zn (s) → Zn2+ (aq) + Pb (s)
2Cr3+
b. 2Cr3+

19. Acids and Bases #1
The
2Cr3+
b. 2Cr3+

20. Acids and Bases #2
The
2Cr3+
b. 2Cr3+

21. Acids and Bases #3
The
2Cr3+
b. 2Cr3+

22. Acids and Bases #4
The
2Cr3+
b. 2Cr3+