Consider the reaction \(2 A _{( g )} \rightleftharpoons B _{( g )}+ C _{( q )}, \Delta H =+25.6 kJ\) Which of the following changes will favour the formation of the products of the reaction represented above, at equilibrium?
A. Decrease in temperature B. Increase in pressure C. Increase in temperature D. Decrease in volume
Correct Answer: C
Explanation
The reaction is endothermic. For endothermic reactions, increasing the temperature favours product formation (forward reaction), while the reverse reaction is favoured by decreasing the temperature. Note that pressure has no effect on the reaction since the net no of mole of gaseous species is zero ( 2 moles on the left, 2 moles on the right).
