Consider the reaction: A + 2B\(_{(g)} \rightleftharpoons \) 2C + D\(_{(g)}\) (\(\Delta\)H = +ve) What will be the effect of decrease in temperature on the reaction?

Consider the reaction: A + 2B\(_{(g)} \rightleftharpoons \) 2C + D\(_{(g)}\) (\(\Delta\)H = +ve)

What will be the effect of decrease in temperature on the reaction?

A Rate of backward reaction will increase
B The equilibrium constant will shift
C Rates of forward and backward reactions are not affected
D Rate of forward reaction will increase

jamb 2019 chemistry

The correct answer is A. Rate of backward reaction will increase

The given reaction is endothermic, hence, a decrease in temperature will favor the exothermic side which is the backward reaction.

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