How can you predict the following stages of a reaction by comparing the value of K_{c} \; and \; Q_{c}?

(i) Net reaction proceeds in the forward direction.

(ii) Net reaction proceeds in the backward direction.

(iii) No net reaction occurs.

Answers (1)

The values of K_{c} (the equilibrium constant) and Q_{c} (the reaction quotient) less than or greater than one another decides the direction in which reaction will proceed as follows-

 (i) As Q_{c} <K_{c}, this implies that in order to reach the equilibrium, the concentration of the products must be increased, hence the reaction will proceed in the forward direction.

(ii) If Q_{c} >K_{c}, this implies that in order to reach the equilibrium, the concentration of the products must be decreased, hence the reaction will proceed in the backward direction.  

(iii) If Q_{c} =K_{c}, no net reaction occurs as the equilibrium has been achieved.

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