Q.When the numerical value of the reaction quotient (Q) is greater than the equilibrium constant (K), in which direction does the reaction proceed to reach equilibrium?

By definition, at equilibrium the reaction quotient Q equals the equilibrium constant K (Q = K), not less than it — so the statement claiming Q < K at equilibrium is false, making it the incorrect statement among the choices.

Check each statement:

1. A catalyst lowers the activation energy for both the forward and reverse reactions by the same amount, so it speeds up both equally without shifting the equilibrium position — this statement is CORRECT.
2. The reaction quotient Q is calculated the same way as K, using the concentrations present at any given moment. When the system reaches equilibrium, by definition Q becomes equal to K (Q = K). Saying Q is 'always less than' K at equilibrium is FALSE — this is the incorrect statement. …

Statement (b) is incorrect because at equilibrium Q always equals K, never remains less than it.

The reaction quotient Q has the same mathematical form as the equilibrium constant K, but Q can be evaluated at ANY point during a reaction using the concentrations present at that instant, whereas K uses the equilibrium concentrations only. Comparing Q to K tells us the direction a reaction will shift: if Q < K the forward reaction proceeds (to increase Q), if Q > K the reverse reaction proceeds, and the reaction reaches equilibrium exactly when Q = K. So the claim that Q is 'always less than' K at equilibrium is wrong — it should be Q = K at equilibrium.

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