In a reaction A2( g)+4 B2( g) ⇌2 AB4( g) ; ΔH<0. The formation of AB4( g) will be favoured by (

step 1 In this problem, we have given a reaction. A2 reacts with 4 mole of B2 gas reversively to give 2

In a reaction A2( g)+4 B2( g) ⇌2 AB4( g) ; ΔH<0. The...

In a reaction $\mathrm{A}_2(\mathrm{~g})+4 \mathrm{~B}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}_4(\mathrm{~g}) ; \Delta \mathrm{H}<0$. The formation of $\mathrm{AB}_4(\mathrm{~g})$ will be favoured by (a) low temperature and high pressure (b) high temperature and high pressure (c) low temperature and low pressure (d) high temperature and low pressure

In a reaction $\mathrm{A}_2(\mathrm{~g})+4 \mathrm{~B}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}_4(\mathrm{~g}) ; \Delta \mathrm{H}<0$. The formation of $\mathrm{AB}_4(\mathrm{~g})$ will be favoured by
(a) low temperature and high pressure
(b) high temperature and high pressure
(c) low temperature and low pressure
(d) high temperature and low pressure

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Key Concepts

Effect of Pressure on Equilibrium in Gaseous Systems

In reactions involving gases, changes in pressure affect the equilibrium by favoring the side with fewer moles of gas. Increasing the pressure will shift the equilibrium toward the side with lower gas volume, thus favoring the formation of products if they consist of fewer moles.

Effect of Temperature on Equilibrium

Temperature changes can shift the equilibrium position of a reaction. For an exothermic reaction, lower temperatures shift the equilibrium towards the products because the reaction releases heat, and reducing temperature minimizes the system's deviation from equilibrium.

Le Chatelier's Principle

This principle explains how a system at equilibrium reacts to disturbances such as changes in temperature or pressure. When a change is imposed, the system shifts its equilibrium position to counteract the disturbance and re-establish equilibrium.

Exothermic Reactions

In an exothermic reaction, heat is released as a product. According to Le Chatelier's principle, lowering the temperature will favor the forward exothermic reaction to produce more heat, thus shifting the equilibrium towards the products.

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