Medium
How can you predict the direction of a reaction by comparing the values of the equilibrium constant $K_{c}$ and the reaction quotient $Q_{c}$?
$(i)$ Net reaction proceeds in the forward direction,
$(ii)$ Net reaction proceeds in the backward direction,
$(iii)$ No net reaction occurs.
$(i)$ Net reaction proceeds in the forward direction,
$(ii)$ Net reaction proceeds in the backward direction,
$(iii)$ No net reaction occurs.
(N/A) The direction of a reaction can be predicted by comparing the reaction quotient $Q_{c}$ with the equilibrium constant $K_{c}$:
$(i)$ If $Q_{c} < K_{c}$,the reaction proceeds in the forward direction (towards products).
$(ii)$ If $Q_{c} > K_{c}$,the reaction proceeds in the backward direction (towards reactants).
$(iii)$ If $Q_{c} = K_{c}$,the reaction is at equilibrium,and no net reaction occurs.
$(i)$ If $Q_{c} < K_{c}$,the reaction proceeds in the forward direction (towards products).
$(ii)$ If $Q_{c} > K_{c}$,the reaction proceeds in the backward direction (towards reactants).
$(iii)$ If $Q_{c} = K_{c}$,the reaction is at equilibrium,and no net reaction occurs.
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