Question

The reaction quotient '$Q$' is useful in predicting the direction of the reaction. Which of the following is incorrect ?

• A. If $Q_c > K_c$, the reverse reaction is favoured
• B. If $Q_c < K_c$, the forward reaction is favoured
• C. If $Q_c = K_c$, no reaction occur
• D. If $Q_c > K_c$, forward reaction is favoured

Answer 1

Answer: (D)

If $Q_c > K_c$, forward reaction is favoured

Answer 2

The direction in which the reaction is expected to proceed

$Q_{c}>K_{c}$ (reaction goes from right to left) In this case, the reaction proceeds in the reverse or the backward direction or in the direction of the reactants.

$Q_{c} < K_{c}$ (the reaction goes from left to right) In this case, the reaction proceeds in the forward direction or the direction of the products.

$Q_{c}=K_{c}$ (reaction is at equilibrium) In this case, the reaction is said to be at equilibrium.

But the reaction is dynamic in nature.