For the following three reactions A, B and C, equilibrium constants are given: [2008] (a) CO(g)+

step 1 In this problem, we have given three reactions with equilibrium constants K1, K2 and K3, and we

For the following three reactions A, B and C, equilibrium...

For the following three reactions $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$, equilibrium constants are given: [2008] (a) $\mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g}) ; \mathrm{K}_{1}$(b) $\mathrm{CH}_{4}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{~g}) ; \mathrm{K}_{2}$ (c) $\mathrm{CH}_{4}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})+4 \mathrm{H}_{2}(\mathrm{~g}) ; \mathrm{K}_{3}$ Which of the following relation is correct? (a) $\mathrm{K}_{1} \sqrt{\mathrm{K}}_{2}=\mathrm{K}_{2}$ (b) $\mathrm{K}_{2} \mathrm{~K}_{3}=\mathrm{K}_{1}$ (c) $\mathrm{K}_{3}=\mathrm{K}_{1} \mathrm{~K}_{2}$ (d) $\mathrm{K}_{3} \cdot \mathrm{K}_{2}^{3}=\mathrm{K}_{1}^{2}$

For the following three reactions $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$, equilibrium constants are given:
[2008]
(a) $\mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g}) ; \mathrm{K}_{1}$(b) $\mathrm{CH}_{4}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{~g}) ; \mathrm{K}_{2}$
(c) $\mathrm{CH}_{4}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})+4 \mathrm{H}_{2}(\mathrm{~g}) ; \mathrm{K}_{3}$
Which of the following relation is correct?
(a) $\mathrm{K}_{1} \sqrt{\mathrm{K}}_{2}=\mathrm{K}_{2}$
(b) $\mathrm{K}_{2} \mathrm{~K}_{3}=\mathrm{K}_{1}$
(c) $\mathrm{K}_{3}=\mathrm{K}_{1} \mathrm{~K}_{2}$
(d) $\mathrm{K}_{3} \cdot \mathrm{K}_{2}^{3}=\mathrm{K}_{1}^{2}$

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state of a reversible reaction in which the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of reactants and products over time. This concept is fundamental in chemistry and is quantified by an equilibrium constant that expresses the ratio of product concentrations to reactant concentrations at equilibrium.

Equilibrium Constant Expression

The equilibrium constant, typically denoted as K, is defined by an expression that relates the concentrations (or partial pressures) of products and reactants, each raised to the power of their respective stoichiometric coefficients. This expression provides a quantitative measure of the extent to which a reaction has proceeded at equilibrium and is central to predicting the direction and yield of a chemical reaction.

Reaction Combination and Equilibrium Constants

When dealing with multiple chemical reactions, it is possible to derive the equilibrium constant for a net reaction by combining individual reactions. A key principle is that if two or more reactions are added together, the equilibrium constant for the overall reaction is the product of the equilibrium constants for the individual reactions. This principle allows one to relate the equilibrium constants of composite reactions to those of the constituent reactions.

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