WAEC - Chemistry (2011 - No. 32)
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
הֶסבֵּר
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.