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- 1. Multiple Choice
An equilibrium constant with a value of 4.6 x 1015 indicates that at equilibrium
the reactants are favored.
the products are favored.
approximately equal concentrations of reactants and products are present.
- 2. Multiple Choice
When pressure decreases, in which direction does the equilibrium shift?
The equilibrium shifts in the direction that increases the number of moles of gas.
The equilibrium shifts in the direction that decreases the number of moles of gas.
The equilibrium does not shift.
The equilibrium shifts always shifts to the right.
The equilibrium shifts always shifts to the left.
- 3. Multiple Choice
For an endothermic reaction, increasing the temperature
does not shift the equilibrium since K is a constant.
increases the rate of the reverse reaction to form more reactants.
increases the rate of the forward reaction to form more products.
increases the rate of the reverse reaction to form more products.
- 4. Multiple Choice
For which of the following reactions does Kp = Kc?
3Fe(s) + 4H2O(g) ⇌ Fe3O4(s) + 4H2(g)
C(s) + H2O(g) ⇌ CO(g) + H2(g)
2SO2(g) + O2(g) ⇌ 2SO3(g)
H2(g) + I2(s) ⇌ 2HI(g)
- 5. Multiple Choice
What is the value for Kc if [CO] = 0.025, [H2] = 0.013 and [CH3OH] = 0.0028 for the following reaction?
CH3OH(g) ⇌ CO(g) + 2 H2(g)
0.12
9.1 × 10-7
6.6 × 102
1.5 × 10-3
8.6
- 6. Multiple Choice
Which of the following substances present in the chemical reaction would NOT be included in the equilibrium constant expression?
solvents
NaCl(s)
H2O(l)
NH4Cl(s)
all of these
- 7. Multiple Choice
For the following chemical equilibrium, Kp = 4.6 × 10-14 at 25 °C, find the value of Kc for this reaction at 25 °C.
2 Cl2(g) + 2 H2O(g) ⇔ 4 HCl(g) + O2(g)
Kc = 2.2 × 10-14
Kc = 4.6 × 10-14
Kc = 9.4 × 10-14
Kc = 1.9 × 10-15
Kc = 1.1 × 10-12
- 8. Multiple Choice
For the reaction PCl5 (g) → PCl3 (g) + Cl2 (g) Kc = 0.0454 at 261°C. If a vessel is filled with these gases such that the initial concentrations are [PCl5] = 0.25M, [PCl3] = 0.20 M, and [Cl2] = 2.25 M, in which direction will a reaction occur and why?
toward products because Q = 0.56
toward reactants because Q = 1.8
it is at equilibrium
toward reactants because Q = 0.0454
toward products because Q = 2.8
- 9. Multiple Choice
Consider the following reaction.
C(s) + H2O(g) ⇌ CO(g) + H2(g)
At equilibrium at a certain temperature, [H2O(g)] = 0.12 M, and [CO(g)] = [H2(g)] = 1.2 M. If suddenly these concentrations are increased by 0.50 M, which of the following is true?
Since Kc does not change, nothing happens.
more products are formed
more H2O(g) will be formed
Kc = 4.66
- 10. Multiple Choice
Then notation [A]4 is equivalent to which of the following?
[A] + [A] + [A] + [A]
[A] × [A] × [A] × [A]
1/([A] + [A] + [A] + [A])
1/([A] × [A] × [A] × [A])
- 11. Multiple Choice
For the reaction: CH4(g) + 2 H2O(g) ⇔ CO2(g) + 4 H2(g) ΔH° = +190 kJ raise the temperature to 1200 K:
the temperature increases.
the ΔH° increases.
the reaction reacts to the right.
the reaction reacts to the left.
there is no change.
- 12. Multiple Choice
In a reaction at equilibrium involving only gases, a change in pressure of the reaction mixture shifts the position of equilibrium only when:
the reaction is exothermic as written
the gases are impure
the collision rate increases
heat is absorbed by the reaction proceeding to the right
the moles of gas are not equal on the two sides of the equation.
- 13. Multiple Choice
For the reaction: 3 Fe(s) + 4 H2O(g) ⇔ Fe3O4(s) + 4 H2(g) what is the effect of removing H2?
The Kp is decreased.
The reaction shifts to the right.
There is no change.
The reaction shifts to the left.
The Kp is doubled.
- 14. Multiple Choice
Consider the reaction: CH4(g) + 4 Cl2(g) ⇔ CCl4(l) + 4 HCl(g) ΔH° -398 kJ/mol The equilibrium is displaced to the right if:
the pressure is lowered
the temperature is raised
some hydrogen chloride is added
some carbon tetrachloride is removed
- 15. Multiple Choice
Choose the correct statement about a container in which the chemical equilibrium is established:
2 SO2(g) + O2(g) → 2 SO3(g) + heat
A decrease in the volume will decrease the amount of SO2 present.
An increase in amount of O2 will increase the amount of SO2 present.
A decrease in temperature will increase the amount of SO2 present.
A decrease in the amount of SO3 present will increase the amount of SO2 present.
A decrease in amount of O2 will decrease the amount of SO2 present.
- 16. Multiple Choice
Consider the following reaction at a certain temperature.
2SO3(g) ⇌ 2SO2(g) + O2(g)
When the initial concentration of SO3(g) is 0.128 M, at equilibrium the concentration of oxygen gas is found to be 0.0130 M. Calculate Kc for this reaction.
8.45 x 10-4
1.47 x 10-3
7.64 x 10-5
1.62 x 10-2
- 17. Multiple Choice
For the formation of NO2, Kc = [NO2]/[NO][O2]1/2. At equilibrium in a 2.50 L container, there are 3.00 mol NO, 4.00 mol O2 and 22.0 mol NO2. The value of Kc is:
13.4
5.80
0.0116
33.6
- 18. Multiple Choice
What is ΔH° for a reaction that has Kp = 1.456 at 273 K and Kp = 14.2 at 298 K?
462 kJ/mol
61.6 kJ/mol
-462 kJ/mol
-61.6 kJ/mol
8.42 × 10-5 kJ/mol
- 19. Multiple Choice
For a reaction Keq = 1.2 × 10-6 at T = 200 K. What is ΔG° for the reaction?
-22.7 kJ/mol
22.7 kJ/mol
53.6 kJ/mol
170 kJ/mol
-53.6 kJ/mol
- 20. Multiple Choice
Calculate the temperature for which Keq for a reaction is 1.04 × 103 where ΔH° = -83.2 kJ/mol and ΔS° = -246 J/mol ∙ K.
0.307 K
307 K
274 K
0.274 K
cannot be determined without ΔG°
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