Deck 13: Fundamental Equilibrium Concepts

Question 1

Consider the following equilibrium mixture in a closed system: H₂Og) + COg) ⇌ H₂g) + CO₂g). Explain what would happen to the equilibrium upon the addition of carbon monoxide gas? Outcome # 3) DOK 3)

A) 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.
B) The addition of carbon monoxide gas would not disrupt the equilibrium, so nothing would happen.
C) 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.

Answer 1

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.

Question 2

Consider the following equilibrium mixture in a closed system: H₂Og) + COg) ⇌ H₂g) + CO₂g). Explain what would happen to the equilibrium upon the addition of hydrogen gas? Outcome # 3) DOK 3)

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.
B) 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.
C) The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen.

Answer 2

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.

Question 3

If the reaction quotient is greater than the equilibrium constant, which statement would be correct? Outcome # 4) DOK 1)

A) If Q > K, then the reaction needs to proceed towards the right to reach equilibrium.
B) If Q > K, then the reaction needs to proceed towards the left to reach equilibrium.
C) If Q > K, then the reaction is at equilibrium.

Answer 3

If Q > K, then the reaction needs to proceed towards the left to reach equilibrium.

Question 4

Write the equilibrium expression for H₂Og) + COg) ⇌ H₂g) + CO₂g). Outcome # 3) DOK 1)

A) K_c = [CO₂] [H₂] / [H₂O] [CO]
B) K_c = [H₂O] [CO] / [CO₂] [H₂]
C) K_c = [CO₂] [H₂] / [CO]

Question 5

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)

A) Q = 5.15 which is less than K_c, therefore the reaction needs to proceed towards the right to reach equilibrium
B) Q = 15.2 which is less than K_c, therefore the reaction needs to proceed towards the right to reach equilibrium
C) Q = 0.194 which is less than K_c, therefore the reaction needs to proceed towards the right to reach equilibrium

Question 6

Write the equilibrium expression for 2NOg) + 2H₂g) ⇌ N₂g) + 2H₂Og). Outcome # 3) DOK 1)

A) K_c = [NO]² [H₂]² / [H₂O]² [N₂]
B) K_c = [H₂O]² [N₂] / [NO]² [H₂]²
C) K_c = [N₂] / [NO]² [H₂]²

Question 7

If the reaction quotient is less than the equilibrium constant, which statement would be correct? Outcome # 4) DOK 1)

A) If Q < K, then the reaction needs to proceed towards the left to reach equilibrium.
B) If Q < K, then the reaction is at equilibrium.
C) If Q < K, then the reaction needs to proceed towards the right to reach equilibrium.