Question

Which of the following is not a result when a change to an equilibrium system is applied? Increasing the rate of the forward reaction will cause a shift to the left. Increasing the rate of the reverse reaction will cause a shift to the left. Decreasing the rate of the forward reaction will cause a shift to the left. Decreasing the rate of the reverse reaction will cause a shift to the right.

Answer 1

Answer: Increasing the rate of the reverse reaction will cause a shift to the left.

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation:

$A+B\leftrightharpoons C+D$

For the given options:

Option A: Increasing the rate of the forward reaction will cause a shift to the left.

If the rate of forward reaction is increased, so according to the Le-Chatelier's principle , the equilibrium will shift in the direction where decrease in forward reaction occurs. Hence, the equilibrium will shift in the left direction.

Option B: Increasing the rate of the reverse reaction will cause a shift to the left.

If the rate of reverse reaction is increased, so according to the Le-Chatelier's principle , the equilibrium will shift in the direction where decrease in reverse reaction occurs. Hence, the equilibrium will shift in the right direction.

Option C: Decreasing the rate of the forward reaction will cause a shift to the left

If the rate of forward reaction is decreased, so according to the Le-Chatelier's principle , the equilibrium will shift in the direction where increase in forward reaction occurs. Hence, the equilibrium will shift in the right direction.

Option D: Decreasing the rate of the reverse reaction will cause a shift to the right.

If the rate of reverse reaction is decreased, so according to the Le-Chatelier's principle , the equilibrium will shift in the direction where increase in reverse reaction occurs. Hence, the equilibrium will shift in the left direction.

From the above explanation, we can easily say that the correct answer is Option B.

Answer 2

2) Increasing the rate of the reverse reaction will cause a shift to the left.

Hopefully, If it is wrong my full apologies.

OR IF THATS WRONG, TRY THIS

a - Increasing the rate of the forward reaction will cause equilibrium to be more product-favored (i.e. shift to the right, not the left)