For the reaction A(g) ⇌ B(g) + C(g), if the concentration of B is increased, wha

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Question: For the reaction A(g) ⇌ B(g) + C(g), if the concentration of B is increased, what will be the effect on the equilibrium? (2020)

Options:

Correct Answer: Shift to the left

Exam Year: 2020

Solution:

Increasing the concentration of B will shift the equilibrium to the left to counteract the change, according to Le Chatelier\'s principle.

For the reaction A(g) ⇌ B(g) + C(g), if the concentration of B is increased, what will be the effect on the equilibrium? (2020)

For the reaction A(g) ⇌ B(g) + C(g), if the concentration of B is increased, what will be the effect on the equilibrium? (2020)

Step 1: Understand that the reaction A(g) ⇌ B(g) + C(g) is in equilibrium, meaning the forward and reverse reactions are happening at the same rate.
Step 2: Recognize that increasing the concentration of B means there is more of B present in the system.
Step 3: Apply Le Chatelier's principle, which states that if a change is made to a system at equilibrium, the system will adjust to counteract that change.
Step 4: Since we increased the concentration of B, the system will try to reduce the amount of B by shifting the equilibrium to the left, which means it will favor the formation of A.
Step 5: Conclude that the effect of increasing the concentration of B is to shift the equilibrium to the left.

Le Chatelier's Principle – This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.