In the reaction, N2+3 H2 ⇌2 NH3+ heat, relationship between Kp and Kc is (a) Kp=Kc(RT)^-2 (b) Kp

step 1 Here in this question we need to tell the relationship between KP and KC. KP and KC that means e

In the reaction, N2+3 H2 ⇌2 NH3+ heat, relationship between...

In the reaction, $\mathrm{N}_2+3 \mathrm{H}_2 \rightleftharpoons 2 \mathrm{NH}_3+$ heat, relationship between $\mathrm{K}_{\mathrm{p}}$ and $\mathrm{K}_{\mathrm{c}}$ is (a) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{-2}$ (b) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^2$ (c) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{e}}(\mathrm{RT})^{-3}$ (d) $\mathrm{K}_{\mathrm{c}}=\mathrm{K}_{\mathrm{p}}(\mathrm{RT})^3$

In the reaction, $\mathrm{N}_2+3 \mathrm{H}_2 \rightleftharpoons 2 \mathrm{NH}_3+$ heat, relationship between $\mathrm{K}_{\mathrm{p}}$ and $\mathrm{K}_{\mathrm{c}}$ is
(a) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{-2}$
(b) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^2$
(c) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{e}}(\mathrm{RT})^{-3}$
(d) $\mathrm{K}_{\mathrm{c}}=\mathrm{K}_{\mathrm{p}}(\mathrm{RT})^3$

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Key Concepts

Equilibrium Constant

The equilibrium constant is a numerical value that indicates the extent to which a chemical reaction proceeds at equilibrium. It is defined by the ratio of the concentrations or partial pressures of products to reactants, each raised to the power of their stoichiometric coefficients. This constant is crucial for predicting the position of equilibrium in chemical reactions.

Kp and Kc Relationship

For gaseous reactions, there is a link between the equilibrium constants expressed in terms of partial pressures (Kp) and concentrations (Kc). This relationship is given by the equation Kp = Kc (RT)^(?n), where R is the ideal gas constant, T is the absolute temperature, and ?n represents the net change in the number of moles of gas during the reaction.

Delta n (?n) Calculation

Delta n (?n) is calculated as the difference between the moles of gaseous products and the moles of gaseous reactants. This value is pivotal in the conversion between Kc and Kp because it determines the power to which the product RT is raised in the relationship, directly influencing how changes in temperature affect the equilibrium constants in gas-phase reactions.

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