Consider the following reaction equation:
X(g) + Y(g) ⇌ XY(g); ∆H = + 220KJ mol-1 If the temperature of the system is increased, the
- backward reaction would be favoured
-
forward reaction would favoured
- reaction would stop
- reaction would be at equilibrium
The correct answer is: B
Explanation
According to Le Chatelier's principle, in an endothermic reaction (whenever delta H = +), an increase in temperature will cause the equilibrium position to shift to the right, thereby leading to the formation of more of the product i.e The forward reaction will be favoured while a decrease in temperature will cause the equilibrium position to shift to the left. Which implies the backward reaction will be favoured. The reverse is the case in an exothermic reaction ( whenever delta H = - ). Therefore, the correct answer is option B.