In which of the following reactions, equilibrium is...

In which of the following reactions, equilibrium is independent of pressure? (a) $\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g}) ; \Delta \mathrm{H}=+$ ve (b) $2 \mathrm{SO}_2+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_3(\mathrm{~g}) ; \Delta \mathrm{H}=-\mathrm{ve}$ (c) $3 \mathrm{H}_2(\mathrm{~g})+\mathrm{N}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}) ; \Delta \mathrm{H}=-\mathrm{ve}$ (d) $\mathrm{PCl}_5(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g}) ; \Delta \mathrm{H}=+$ ve

In which of the following reactions, equilibrium is independent of pressure?
(a) $\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g}) ; \Delta \mathrm{H}=+$ ve
(b) $2 \mathrm{SO}_2+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_3(\mathrm{~g}) ; \Delta \mathrm{H}=-\mathrm{ve}$
(c) $3 \mathrm{H}_2(\mathrm{~g})+\mathrm{N}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}) ; \Delta \mathrm{H}=-\mathrm{ve}$
(d) $\mathrm{PCl}_5(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g}) ; \Delta \mathrm{H}=+$ ve

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Key Concepts

Chemical Equilibrium

This concept refers to the state in which the rate of the forward reaction equals the rate of the reverse reaction. At equilibrium, the concentrations of reactants and products remain constant over time, although both reactions continue to occur. Understanding chemical equilibrium is essential for explaining how reactions respond to changes in conditions such as pressure, temperature, and concentration.

Le Chatelier's Principle

Le Chatelier's Principle is a fundamental concept that predicts how a system at equilibrium will react to a disturbance. If an external change is applied—such as a change in pressure, temperature, or concentration—the system will adjust in a way that counteracts that change. This principle is key to understanding why and how equilibrium positions shift when conditions are altered.

Moles of Gas and Pressure Dependence

In gas-phase reactions, the effect of pressure on the equilibrium state is determined by the difference in the number of moles of gaseous reactants and products. When the total number of moles of gas is the same on both sides of the reaction, altering the pressure does not favor either direction, making the equilibrium independent of pressure changes. Conversely, if there is a difference, pressure changes will shift the equilibrium in the direction that minimizes the change.

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