Chapter 13 Fundamental Equilibrium Concepts Full Test Bank

Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 13: Fundamental Equilibrium Concepts

1. Consider the following equilibrium mixture in a closed system: H₂O(g) + CO(g) ⇌ H₂(g) + CO₂(g). Explain what would happen to the equilibrium upon the addition of hydrogen gas? (Outcome # 3) (DOK 3)
   1. The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved.
   2. The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right which would result in more CO₂ being produced until equilibrium is achieved.
   3. The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen.
2. Consider the following equilibrium mixture in a closed system: H₂O(g) + CO(g) ⇌ H₂(g) + CO₂(g). Explain what would happen to the equilibrium upon the addition of carbon monoxide gas? (Outcome # 3) (DOK 3)
3. The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved.
4. The addition of carbon monoxide gas would not disrupt the equilibrium, so nothing would happen.
5. The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the right which would result in more products being produced until equilibrium is achieved.
6. Write the equilibrium expression for H₂O(g) + CO(g) ⇌ H₂(g) + CO₂(g). (Outcome # 3) (DOK 1)
7. K_c = [CO₂] [H₂] / [H₂O] [CO]
8. K_c = [H₂O] [CO] / [CO₂] [H₂]
9. K_c = [CO₂] [H₂] / [CO]
10. Write the equilibrium expression for 2NO(g) + 2H₂(g) ⇌ N₂(g) + 2H₂O(g). (Outcome # 3) (DOK 1)
11. K_c = [NO]² [H₂]² / [H₂O]² [N₂]
12. K_c = [H₂O]² [N₂] / [NO]² [H₂]²
13. K_c = [N₂] / [NO]² [H₂]²
14. The K_c for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, I₂, and H₂ are 0.338 M, 0.112 M, and 0.198 M respectively, which statement is correct? (Outcome # 4) (DOK 2)
15. Q = 5.15 which is less than K_c, therefore the reaction needs to proceed towards the right to reach equilibrium
16. Q = 15.2 which is less than K_c, therefore the reaction needs to proceed towards the right to reach equilibrium
17. Q = 0.194 which is less than K_c, therefore the reaction needs to proceed towards the right to reach equilibrium
18. If the reaction quotient is greater than the equilibrium constant, which statement would be correct? (Outcome # 4) (DOK 1)
19. If Q > K, then the reaction needs to proceed towards the right to reach equilibrium.
20. If Q > K, then the reaction needs to proceed towards the left to reach equilibrium.
21. If Q > K, then the reaction is at equilibrium.
22. If the reaction quotient is less than the equilibrium constant, which statement would be correct? (Outcome # 4) (DOK 1)
23. If Q < K, then the reaction needs to proceed towards the left to reach equilibrium.
24. If Q < K, then the reaction is at equilibrium.
25. If Q < K, then the reaction needs to proceed towards the right to reach equilibrium.