At constant temperature, the equilibrium constant (Kp) for the decomposition reaction, N2 O4 ⇄2

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At constant temperature, the equilibrium constant (Kp) for...

At constant temperature, the equilibrium constant $\left(\mathrm{K}_{\mathrm{p}}\right)$ for the decomposition reaction, $\mathrm{N}_2 \mathrm{O}_4 \rightleftarrows 2 \mathrm{NO}_2$ is expressed by $K_p=\left(4 x^2 P\right) /\left(1-x^2\right)$, where $P=$ pressure, $x=$ extent of decomposition. Which one of the following statements is true? (a) $\mathrm{K}_{\mathrm{p}}$ increases with increase of P (b) $\mathrm{K}_{\mathrm{p}}$ increases with increase of $x$ (c) $\mathrm{K}_{\mathrm{p}}$ increases with decrease of $x$ (d) $\mathrm{K}_{\mathrm{p}}$ remains constant with change in P and x

At constant temperature, the equilibrium constant $\left(\mathrm{K}_{\mathrm{p}}\right)$ for the decomposition reaction, $\mathrm{N}_2 \mathrm{O}_4 \rightleftarrows 2 \mathrm{NO}_2$ is expressed by
$K_p=\left(4 x^2 P\right) /\left(1-x^2\right)$, where $P=$ pressure, $x=$ extent of decomposition. Which one of the following statements is true?
(a) $\mathrm{K}_{\mathrm{p}}$ increases with increase of P
(b) $\mathrm{K}_{\mathrm{p}}$ increases with increase of $x$
(c) $\mathrm{K}_{\mathrm{p}}$ increases with decrease of $x$
(d) $\mathrm{K}_{\mathrm{p}}$ remains constant with change in P and x

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. This concept is critical because it explains how reactions can reach a stable state and how the composition of the system is maintained over time.

Equilibrium Constant

The equilibrium constant is a ratio of the concentrations (or partial pressures, in the case of gases) of products to reactants at equilibrium, raised to the power of their stoichiometric coefficients. At constant temperature, this constant remains unchanged regardless of changes in pressure or extent of reaction, indicating the inherent balance of the reaction under specific thermodynamic conditions.

Partial Pressure in Gaseous Equilibria

Partial pressure is the pressure exerted by a single gas component in a mixture. In gaseous equilibrium systems, equilibrium expressions like Kp are written in terms of partial pressures, linking the amount of each gaseous species to the overall equilibrium state of the reaction.

Extent of Reaction

The extent of reaction quantifies the progress of a reaction by expressing the degree to which reactants have been converted into products. It is a useful parameter in equilibrium expressions as it helps relate the observable changes in system conditions, such as pressure, to the equilibrium constant when reactions involve gases.

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