Equilibrium constants K1, and K2 for the following equilibria NO(g)+1 / 2 O2 K1 NO2( g) and are

step 1 In this problem we have given that equilibrium constants K1 and K2 for the following equilibrium

Equilibrium constants K1, and K2 for the following...

Equilibrium constants $\mathrm{K}_1$, and $\mathrm{K}_2$ for the following equilibria $\mathrm{NO}(\mathrm{g})+1 / 2 \mathrm{O}_2 \xlongequal{\mathrm{~K}_1} \mathrm{NO}_2(\mathrm{~g})$ and are related as (a) $\mathrm{K}_2=1 / \mathrm{K}_1^2$ (b) $\mathrm{K}_2=\mathrm{K}_1^2$ (c) $\mathrm{K}_2=1 / \mathrm{K}_1$ (d) $\mathrm{K}_2=\mathrm{K}_1 / 2$

Equilibrium constants $\mathrm{K}_1$, and $\mathrm{K}_2$ for the following equilibria
$\mathrm{NO}(\mathrm{g})+1 / 2 \mathrm{O}_2 \xlongequal{\mathrm{~K}_1} \mathrm{NO}_2(\mathrm{~g})$ and
are related as
(a) $\mathrm{K}_2=1 / \mathrm{K}_1^2$
(b) $\mathrm{K}_2=\mathrm{K}_1^2$
(c) $\mathrm{K}_2=1 / \mathrm{K}_1$
(d) $\mathrm{K}_2=\mathrm{K}_1 / 2$

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Key Concepts

Equilibrium Constant

The equilibrium constant is a quantitative measure of the position of equilibrium in a chemical reaction. It is defined as the ratio of the concentrations or partial pressures of the products to those of the reactants, each raised to the power of their stoichiometric coefficients. This concept is central in chemical thermodynamics, as it helps predict the extent to which a reaction will proceed under given conditions.

Reaction Manipulation Rules

When chemical reactions are reversed, added, or multiplied by a factor, the overall equilibrium constant changes in a predictable way. For example, if a reaction is multiplied by a factor, the new equilibrium constant becomes the original constant raised to that power, and if two reactions are added together, the equilibrium constant for the overall reaction is the product of the individual constants. These manipulation rules allow us to relate and compute equilibrium constants for reactions derived from combining or modifying other reactions.

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