A2( g)+B2( g) ⇌2 AB(g) ; ΔH=+ve, it (a) increase by pressure (b) it occurs at 1000 atm pressure

step 1 In this problem, we have given that A2 reacts with B2 reversibly and gives 2 moles of AB. And de

A2( g)+B2( g) ⇌2 AB(g) ; ΔH=+ve, it (a) increase by pressure...

$\mathrm{A}_2(\mathrm{~g})+\mathrm{B}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g}) ; \Delta \mathrm{H}=+\mathrm{ve}$, it
(a) increase by pressure
(b) it occurs at 1000 atm pressure
(c) it occurs at high temperature
(d) it occurs at high pressure and temperature

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Key Concepts

Effect of Temperature on Endothermic Reactions

Temperature plays a crucial role in determining the equilibrium position of a reaction. For endothermic reactions, which absorb heat (indicated by a positive ?H), an increase in temperature shifts the equilibrium toward the product side to absorb the additional heat. This principle is essential for understanding how thermal energy influences reaction dynamics and equilibrium states.

Effect of Pressure on Gaseous Equilibria

For reactions involving gases, changes in pressure can significantly affect the equilibrium position. Increasing the pressure typically favors the side of the reaction with fewer moles of gaseous species, as this reduces the overall pressure of the system. This concept is critical in predicting how gaseous equilibria respond to changes in volume and pressure.

Le Chatelier's Principle

Le Chatelier's Principle is a fundamental concept in chemical equilibrium which states that if a dynamic equilibrium is disturbed by changing the conditions, the system responds by counteracting the change to re-establish equilibrium. In reactions involving gases, changes in pressure or temperature can shift the equilibrium position toward the side with fewer or more moles of gas, or favor either the endothermic or exothermic direction, in order to minimize the applied stress.

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