Match the following Column-I (a) N2 O4( g) ⟼2 NO2( g) (b) PCl3( g) ⇌PCl3( g)+Cl2( g) (c) NH2 COO

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Match the following Column-I (a) N2 O4( g) ⟼2 NO2( g) (b)...

Match the following Column-I (a) $\mathrm{N}_2 \mathrm{O}_{4(\mathrm{~g})} \longmapsto 2 \mathrm{NO}_{2(\mathrm{~g})}$ (b) $\mathrm{PCl}_{3(\mathrm{~g})} \rightleftharpoons \mathrm{PCl}_{3(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})}$ (c) $\mathrm{NH}_2 \mathrm{COONH}_{4(\mathrm{~s})} \rightleftharpoons 2 \mathrm{NH}_{3(\mathrm{~g})}+\mathrm{CO}_{2(\mathrm{~g})}$ (d) $\mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{HI}_{\text {(g) }}$ Column-II (p) $K_p=\frac{4 x^2 P}{a^2-x^2}$ (q) $\mathrm{K}_{\mathrm{P}}=\frac{4 \mathrm{P}^3}{27}$ (r) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}$ (s) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}$. RT (t) $\Delta \mathrm{ng}_{\mathrm{g}}>0$

Match the following

Column-I
(a) $\mathrm{N}_2 \mathrm{O}_{4(\mathrm{~g})} \longmapsto 2 \mathrm{NO}_{2(\mathrm{~g})}$
(b) $\mathrm{PCl}_{3(\mathrm{~g})} \rightleftharpoons \mathrm{PCl}_{3(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})}$
(c) $\mathrm{NH}_2 \mathrm{COONH}_{4(\mathrm{~s})} \rightleftharpoons 2 \mathrm{NH}_{3(\mathrm{~g})}+\mathrm{CO}_{2(\mathrm{~g})}$
(d) $\mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{HI}_{\text {(g) }}$

Column-II
(p) $K_p=\frac{4 x^2 P}{a^2-x^2}$
(q) $\mathrm{K}_{\mathrm{P}}=\frac{4 \mathrm{P}^3}{27}$
(r) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}$
(s) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}$. RT
(t) $\Delta \mathrm{ng}_{\mathrm{g}}>0$

Key Concepts

Effect of Phases on Equilibrium Expressions

In equilibrium expressions, only the concentrations or partial pressures of species in the gaseous or aqueous phase are usually included. Phases such as pure solids and liquids are omitted because their activities are constant. This principle simplifies the formulation of equilibrium expressions for complex reactions.

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction, leading to stable concentrations or pressures of reactants and products. This concept is essential for analyzing how reactions adjust to changes in conditions such as pressure, temperature, or concentration.

Equilibrium Constants (Kp and Kc)

Equilibrium constants quantify the extent to which a reaction proceeds to form products at equilibrium. For gaseous reactions, Kp is expressed in terms of the partial pressures of gases, while Kc is expressed in terms of their molar concentrations. These constants are fundamental for predicting the composition of the reaction mixture at equilibrium.

Relationship between Kp and Kc

The relationship between Kp and Kc for gas-phase equilibria is given by the equation Kp = Kc (RT)^(?n), where R is the gas constant, T is the temperature, and ?n is the difference in moles of gaseous products and reactants. This relationship allows the conversion between concentration-based and pressure-based equilibrium constants, highlighting the influence of mole changes on equilibrium.

Reaction Stoichiometry and Change in Moles

Reaction stoichiometry determines the change in the number of moles of gas (?n) during a chemical reaction. This change is critical for understanding how equilibrium positions respond to variations in pressure or volume and plays a key role in the relationship between Kp and Kc. An increase in the number of gas moles typically affects the system’s response under changing conditions.

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