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

${\mathrm{Q}}_{\mathrm{c}}>{\mathrm{K}}_{\mathrm{c}}$, reverse reaction is favored. The product concentration is more than the equilibrium concentration. The reactant concentration is less than the equilibrium concentration.

If ${\mathrm{Q}}_{\mathrm{c}}<{\mathrm{K}}_{\mathrm{c}}$ forward reaction is favored.

If ${\mathrm{Q}}_{\mathrm{c}}={\mathrm{K}}_{\mathrm{c}}$ the reaction is at equilibrium that is dynamic. Both forward and reverse reactions continue to occur.

Hence the correct answer (D) If $Q_c=K_c$, no reaction occur