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
Correct Answer: A
Explanation
The given reaction is endothermic, hence, a decrease in temperature will favor the exothermic side which is the backward reaction.
