Question

Which of the following is not a result when a change to an equilibrium system is applied? (2 points)

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

It should be increasing the rate of the forward reaction will cause a shift to the left because the external stress, which is the increase in rate, will cause the reaction to be unbalanced, and to reach equilibrium it needs to shift to the right.

Answer 2

Answer: Option (2) is the correct answer.

Step-by-step explanation:

According to LeChatelier principle, any change in the equilibrium of a chemical reaction will result in shifting of equilibrium which is opposing the change.

Therefore, when we increase the rate of the reverse reaction that is, we move towards left side then this will actually cause a shift to the right hand side which is opposing the change.

Thus, we can conclude that increasing the rate of the reverse reaction will cause a shift to the left is not a result when a change to an equilibrium system is applied.