The relation between Kp and Kc for the reaction 2 NO(g)+Cl2( g) ⇌2 NOCl(g) is (a) Kp=Kc(RT)^-1 (

step 1 Hello, good evening student. So in this question we have to find the relation between KP and KC

The relation between Kp and Kc for the reaction 2...

The relation between $\mathrm{K}_{\mathrm{p}}$ and $\mathrm{K}_{\mathrm{c}}$ for the reaction $2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NOCl}(\mathrm{g})$ is (a) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{-1}$ (b) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}$ (c) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} /(\mathrm{RT})^2$ (d) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} / \mathrm{RT}$

The relation between $\mathrm{K}_{\mathrm{p}}$ and $\mathrm{K}_{\mathrm{c}}$ for the reaction $2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NOCl}(\mathrm{g})$ is
(a) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{-1}$
(b) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}$
(c) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} /(\mathrm{RT})^2$
(d) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} / \mathrm{RT}$

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Key Concepts

Change in Moles of Gas (?n)

?n is the difference between the sum of the stoichiometric coefficients of the gaseous products and that of the gaseous reactants. This value is crucial in determining the exponent in the equation that relates Kp and Kc. It essentially captures the net change in the number of gas molecules as the reaction proceeds, directly affecting how the equilibrium constant value shifts with temperature and pressure.

Equilibrium Constant Expressions

In chemical equilibrium, different expressions are used depending on whether the concentration of reactants and products or their partial pressures is considered. Kc is defined in terms of molar concentrations while Kp is defined using the partial pressures of gaseous components. These expressions are central to understanding how equilibrium is maintained between reactants and products in a chemical reaction.

Relation between Kp and Kc

The two types of equilibrium constants are related through the equation Kp = Kc(RT)^?n. This relation is derived from the ideal gas law, which connects the concentration of a gas with its pressure. It highlights how the equilibrium behavior in gas-phase reactions is influenced by both concentration and temperature, allowing one to convert between Kc and Kp when needed.

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