Question

Consider the reaction H2(g) + I2(g) <---> HI(g) with an equilibrium constant of 46.3 and a reaction quotient of 525. Which direction will the system shift to?
A. The equilibrium will shift to the left to favor the reactants.
B. The equilibrium will shift to the right to favor the products.
C. The equilibrium will not shift in any direction.
D. The equilibrium will shift to the forward reaction.

Answer 1

Answer:

The equilibrium will shift to the left to favor the reactants.

Explanation:

Remember that the reaction quotient (Qc) is derived from initial concentrations of reactants and products. Since Qc is greater than Kc, this means that initial concentrations are heavily impacted by a high product concentration ([HI]). Therefore, the reverse reaction will occur and actually create more reactants again ([H2] and [I2]). Thus, the answer is that the equilibrium will shift to the left side to favor the reactants.

Answer 2

Answer:

A. The equilibrium will shift to the left to favor the reactants.

Explanation:

Step 1: Data given

K = 46.3

Q = 525

Step 2: The balanced equation

H2(g) + I2(g) <---> HI(g)

When Q=K, the system is at equilibrium and there is no shift to either the left or the right.

When Q<K, there are more reactants than products. As a result, some of the reactants will become products, causing the reaction to shift to the right.

When Q>K, there are more products than reactants. To decrease the amount of products, the reaction will shift to the left and produce more reactants.

For this equation Q >> K

This means there are more products than reactants. To decrease the amount of products, the reaction will shift to the left and produce more reactants.

A. The equilibrium will shift to the left to favor the reactants.