1. Consider the following reaction at equilibrium: 2CO 2 (g) ⇄ 2CO (g) + O 2 (

Question

1. Consider the following reaction at equilibrium:

2CO2 (g) ⇄ 2CO (g) + O2 (g) ΔH ° = −514 kJ

Le Chatelier's principle predicts that an increase in temperature will __________. A) increase the partial pressure of O2 (g)
B) decrease the partial pressure of CO2 (g)
C) decrease the value of the equilibrium constant
D) increase the value of the equilibrium constant
E) increase the partial pressure of CO
2. Nickel (II) oxide reacts with carbon monoxide to form nickel metal.

CO(g) + NiO(s) ⇄ CO2(g) + Ni(s) Kp = 20 at 873 K

If the reaction vessel contains some solid Ni and NiO, 400 mm Hg of CO2 and 20 mm Hg of CO, all at equilibrium, doubling the amount of CO(g) present will lead to the reduction of more nickel oxide at 873 K. A) True
B) False
3. Methanol is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen:

CO(g) + 2 H2(g) ⇄ CH3OH(g)

An equilibrium mixture in a 2.00-L vessel is found to contain 0.0406 mol CH3OH, 0.170 mol CO, and 0.302 mol H2 at 500 K. What is Kp at this temperature? A) 6.22 x 10−3
B) 4.22 x 10−2
C) 0.57
D) 4.65
E) 10.5
4. At 1050 K, Kp = 0.900 for the following reaction:

H2(g) + CO2(g) ⇄ H2O(g) + CO(g)

If 0.200 atm of H2 and 0.200 atm of CO2 are admitted into a rigid container and allowed to reach equilibrium, what should the equilibrium partial pressure of CO be (in atm)?
[enter number with three decimal places]
5. At high temperatures one mole of hydrogen gas reacts with one mole of bromine gas to form hydrogen bromide. At a given temperature the equilibrium constant is 57.6. If at the same temperature, a mixture of 4.67 x 10−3 M hydrogen gas, 2.14 x 10−3 bromine gas, and 2.40 x 10−2 M hydrogen bromide gas is made, then A) the system is far from equilibrium and will shift to form more hydrogen gas.
B) the system is far from equilibrium and will shift to form more hydrogen bromide gas.
C) nothing can be deduced since we do not know whether the reaction is endothermic or exothermic.
D) nothing can be deduced since we do not know whether the equilibrium constant is Kc or Kp.
E) the system is at equilibrium.
6. At 50oC, Kc = 2.2 x 103 for the reaction

3 Fe (s) + 4 H2O (g) ⇄ Fe3O4 (s) + 4 H2 (g)

What is the value of Kp at 200oC for this reaction? A) 8.8 x 103
B) 2.2 x 103
C) 5.5 x 102
D) 3.5 x 104
E) This question cannot be answered with the information provided

Explanation / Answer

1.D

2.B

3.C

4.E

5.A

6.B

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