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Which one of the following conditions will favour maximum formation of the product in the reaction, $A_2(g) + B_2(g) \rightleftharpoons X_2(g)$; $\Delta_rH = -X$ kJ?
Explanation
Exothermic reaction with decrease in gas moles is favoured by low T and high P.
Detailed Solution
$A_2(g) + B_2(g) \rightleftharpoons X_2(g)$; $\Delta H = -X$ kJ
On increasing pressure, equilibrium shifts in the direction where pressure decreases, i.e. the forward direction.
On decreasing temperature, equilibrium shifts in the exothermic direction, i.e. the forward direction.
So high pressure and low temperature favour maximum formation of product.