Which one of the following conditions will favour maximum formation of the product in the reaction, A 2 ( q ) + B 2 ( q ) ⇌ X 2 ( g ) put ; Δ r H = − X kJ?

Step-by-step solution

Using Le-chatlier Principle A 2 ( g ) + B 2 ( g ) ⇌ X 2 ( g ) Δ H = - X KJ On increasing pressure, equilibrium shifts in a direction where volume or number of gaseous moles decreases, i.e., in forward direction here. On decreasing temperature, equilibrium shifts in exothermic direction, i.e., forward direction as heat is coming out of system so decrease of temperature is needed. Hence, high pressure and low temperature favours maximum formation of product in it.