For an equilibrium reaction, which of the following statements is/are correct ?

Options

A. If the reaction quotient of a reaction is greater than `K_(eq)`, the reaction has a tendency to move in the backward direction.
B. If the reaction quotient of a reaction is greater than `K_(eq)`, the reaction has a tendency to the move in the forward direction.
C. The addition of an inert gas at constant volume does not affect the extent of reaction
D. The addition of an inert gas at constant pressure does not affect the extent of reaction.

Answer

A, C, D

Explanation

If the reaction quotient is greater than equilibrium constant, this implies that the products are more than those a equilibrium. Hence, the reaction proceeds in the backward direction.