Title: Chapter 13: Fundamental Equilibrium Concepts
Course: Test

Q: Consider the following equilibrium mixture in a closed system: H_2O(g) + CO(g) ⇌ H_2(g) + CO_2(g). Explain what would happen to the equilibrium upon the addition of hydrogen gas?
- 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.
- The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right which would result in more CO_2 being produced until equilibrium is achieved.
- The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen.
A: 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.

Q: Consider the following equilibrium mixture in a closed system: H_2O(g) + CO(g) ⇌ H_2(g) + CO_2(g). Explain what would happen to the equilibrium upon the addition of carbon monoxide gas?
- 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.
- The addition of carbon monoxide gas would not disrupt the equilibrium, so nothing would happen.
- 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.
A: 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.

Q: Write the equilibrium expression for H_2O(g) + CO(g) ⇌ H_2(g) + CO_2(g).
- K_c = [CO_2] [H_2] / [H_2O] [CO]
- K_c = [H_2O] [CO] / [CO_2] [H_2]
- K_c = [CO_2] [H_2] / [CO]
A: K_c = [CO_2] [H_2] / [H_2O] [CO]

Q: Write the equilibrium expression for 2NO(g) + 2H_2(g) ⇌ N_2(g) + 2H_2O(g).
- K_c = [NO]^2 [H_2]^2 / [H_2O]^2 [N_2]
- K_c = [H_2O]^2 [N_2] / [NO]^2 [H_2]^2
- K_c = [N_2] / [NO]^2 [H_2]^2
A: K_c = [H_2O]^2 [N_2] / [NO]^2 [H_2]^2

Q: The K_c for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, I_2, and H_2 are 0.338 M, 0.112 M, and 0.198 M respectively, which statement is correct?
- Q = 5.15 which is less than K_c, therefore the reaction needs to proceed towards the right to reach equilibrium
- Q = 15.2 which is less than K_c, therefore the reaction needs to proceed towards the right to reach equilibrium
- Q = 0.194 which is less than K_c, therefore the reaction needs to proceed towards the right to reach equilibrium
A: Q = 5.15 which is less than K_c, therefore the reaction needs to proceed towards the right to reach equilibrium

Q: If the reaction quotient is greater than the equilibrium constant, which statement would be correct?
- If Q > K, then the reaction needs to proceed towards the right to reach equilibrium.
- If Q > K, then the reaction needs to proceed towards the left to reach equilibrium.
- If Q > K, then the reaction is at equilibrium.
A: If Q > K, then the reaction needs to proceed towards the left to reach equilibrium.

Q: If the reaction quotient is less than the equilibrium constant, which statement would be correct?
- If Q < K, then the reaction needs to proceed towards the left to reach equilibrium.
- If Q < K, then the reaction is at equilibrium.
- If Q < K, then the reaction needs to proceed towards the right to reach equilibrium.
A: If Q < K, then the reaction needs to proceed towards the right to reach equilibrium.