| 1. Which of the following is the equilibrium constant, K, at 25°C for the Haber process:3 H2(g) + N2(g)→ 2 NH3(g) if the equilibrium concentrations are [H2] = 0.85 M, [N2] = 1.33 M, [NH3] = 0.22 M.
a. 0.059
b. 16.95
c. 0.194
d. 5.139
e. 0.786
2. Which of the following would NOT be able to achieve an equilibrium state?
a. Salt dissolving in water.
b. Boiling water in an open pan
c. Nitrogen dioxide and dinitrogen tetroxide placed in a sealed flask
d. Mixing an acid and a base
e. All would be able to achieve an equilibrium state
3. When dinitrogen tetroxide is placed in a flask at a beginning concentration of 1.0 M at 298 K and allowed to come to equilibrium with nitrogen dioxide according to the reactionN2O4 (g) → 2 NO2(g) the equilibrium concentration of the N2O4 is 0.82 M. What is the equilibrium concentration of the NO2?
a. 0.18 M
b. 0.36 M
c. 0.82 M
d. 0.41 M
e. 1.64 M
4. Which of the following equations represents solubility equilibrium?
a. BaSO2(g) → Ba+2(aq) + S04-2(aq)
b. CH3OH(l) → CH3OH (g)
c. HCl(aq) + H2O (l) → H3O+(aq) + Cl-(aq)
d. C6H12O6(s) → C6H12O6(aq)
e. none of the above
5. For the reaction:CaCO3O (s) → CaO (s) + CO2(g) which of the following is the correct equilibrium expression?
a. K = [CaCO3] / [CaO][CO2]
b. K = [CaO][CO2] / [CaCO3]
c. K = 1 / [CO2]
d. K = [CO2]
e. K = [CaCO3] / [CaO]
6. For the following reaction:heat + 2 NO2 (g) → N2O4 (g) which change will NOT be effective in increasing the amount of N2O4?
a. decreasing the vollume of the reaction
b. increasing the temperature
c. adding nitrogen to increase the pressure
d. adsorbing the N2O4 with a solid adsorbant
e. adding more NO2 to the reaction vessel
7. What is the equilibrium constant for the reaction:COCl2O (g) → CO (g) + Cl2(g) if the concentrations at equilibrium are [CO] = 0.045 M, [Cl2] = 0.045 M, and [COCl2] = 0.500 M?
a. 9.0 x 10-2 M
b. 1.1 x 102 M
c. 4.1 x 10-3 M
d. 2.5 x 102 M
e. 8.1 x 10-3 M
8. If for the reaction:CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g) units were used for the equilibrium constant, K, the units would be which of the following?
a. no units
b. M2
c. M-2
d. M-1
e. M
9. Consider the reaction:2NOCl (g) → 2 NO (g) + Cl2 (g) in the the equilibrium constant, K, is 1.6 x 10-5. If 1.0 mol of pure NOCl and 1.0 mol of pure Cl2 are placed in a 1.0 L container, and x moles of NOCl react
a. which of the following will be the equilibrium concentration of NO?
b. +2x
c. +x
d. -x
e. -2x
10. From the reaction and conditions in the above question, if x moles of NOCl react, which of the following represents the equilibrium concentration of Cl2?
a. +x
b. +x/2
c. 1 + x
d. 1 + x/2
e. 1 + 2x
11. For the hypothetical reaction:2 A (g) + B (g) → C (g) 3.00 mol of A and 4.00 mol of B are placed in a 5.00 L container. At equilibrium, the concentration of A is 0.40 M. Which of the following is the value of K?
a. 0.89
b. 1.80
c. 2.00
d. 3.00
e. none of these
12. At 500°C the equilibrium constant for the reaction:H2 (g) + I2 (g) → 2 HI (g) is 45.0 if 0.3 mol of hydrogen and iodine each are placed into a 10.0 L containiner and allowed to react, what is the hydrogen iodide concentration at equilibrium?
a. 0.0520
b. 0.0926
c. 0.0231
d. 0.0463
e. none of these
13. The correct form for the solubility product for silver chromate would be which of the following?
a. [Ag+]2[CrO4-]
b. [Ag+][CrO4-]
c. [Ag+][CrO4-]2
d. [Ag+]2[CrO4-]4
e. [Ag]2[CrO4]
14. For the equilibriumH2 (g) + CO2 (g) → H2O (g) + CO (g) ΔH = +40kJ If the temperature of the reaction is increased, the equilibrium will shift:
a. left
b. right
c. no change
d. not enough information
e. cannot be determined
15. Keq = 2.5 X 10-9 M2 at 298 K for the following equilibrium reaction. What is the equilibrium concentration of H2 if NH3, initially at 25 mM, is allowed to come to equilibrium at 298 K?2 NH3(g) → N2(g) + 3 H2(g)
a. 6.3 X 10-8 mM
b. 0.49 mM
c. 3.7 mM
d. 1.9 M
e. 2.1 x 10-3 mM
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