For the reaction N2( g)+3 H2( g) ⇌2 NH3( g), ΔH=-93.6 kJ mol^-1, the concentration of H2 at eq

step 1 In this problem, we have given a reaction in 2 gas reacts with 3 moles of H2 gas reversibly to g

For the reaction N2( g)+3 H2( g) ⇌2 NH3( g), ΔH=-93.6 kJ...

For the reaction $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}), \Delta \mathrm{H}=-93.6 \mathrm{~kJ} \mathrm{~mol}^{-1}$, the concentration of $\mathrm{H}_2$ at equilibrium can be increased by (i) lowering the temperature (ii) increasing the volume of the system (iii) adding $\mathrm{N}_2$ at constant volume (iv) adding $\mathrm{H}_2$ at constant volume (a) (ii) and (iv) are correct (b) only (ii) is correct (c) (i), (ii) and (iii) are correct (d) (iii) and (iv) are correct

For the reaction $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}), \Delta \mathrm{H}=-93.6 \mathrm{~kJ} \mathrm{~mol}^{-1}$, the concentration of $\mathrm{H}_2$ at equilibrium can be increased by
(i) lowering the temperature
(ii) increasing the volume of the system
(iii) adding $\mathrm{N}_2$ at constant volume
(iv) adding $\mathrm{H}_2$ at constant volume
(a) (ii) and (iv) are correct
(b) only (ii) is correct
(c) (i), (ii) and (iii) are correct
(d) (iii) and (iv) are correct

Key Concepts

Le Chatelier's Principle

This principle states that if a dynamic equilibrium is disturbed by changing the conditions (such as concentration, pressure, or temperature), the system adjusts itself to counteract the disturbance and re-establish equilibrium. It is used to predict the direction in which the equilibrium will shift when the system is subjected to a change in conditions.

Volume and Pressure Effects on Gaseous Equilibrium

For reactions involving gases, a change in volume (or pressure) affects the equilibrium position. An increase in volume reduces the overall pressure of the system, and according to Le Chatelier's Principle, the equilibrium will shift toward the side with a greater number of moles of gas in order to oppose the change. This concept is crucial in predicting how equilibrium concentrations of gaseous reactants and products will change when the volume of the reaction vessel is altered.

Temperature Effects on Equilibrium

Temperature changes can affect the position of equilibrium depending on whether the reaction is exothermic or endothermic. In exothermic reactions, lowering the temperature effectively removes heat, prompting the equilibrium to shift in the direction that produces heat (the exothermic direction) in order to restore balance. Conversely, raising the temperature favors the endothermic direction. This principle underpins how temperature changes alter reactant and product concentrations at equilibrium.

Effect of Addition of Reactants on Equilibrium

Adding more of a reactant disturbs the equilibrium by increasing its concentration. According to Le Chatelier's Principle, the system will respond by shifting the equilibrium to consume the added reactant and counteract the change. The specific influence on the concentration of other reactants or products depends on the stoichiometry and interrelation of species in the equilibrium system.

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