The equilibrium constant (K) for the reaction N2( g)+O2( g) →2 NO(g) at temperature T is 4 ×10^-

step 1 In this problem we have given that N2 gas reacts with O2 gas reversively to give 2 moles of NO g

The equilibrium constant (K) for the reaction N2( g)+O2( g)...

The equilibrium constant $(\mathrm{K})$ for the reaction $\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NO}(\mathrm{g})$ at temperature T is $4 \times 10^{-4}$. The value of $\mathrm{K}_{\mathrm{c}}$ for the reaction, $\mathrm{NO}(\mathrm{g}) \rightarrow \frac{1}{2} \mathrm{~N}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g})$ at the same temperature is [2012] (a) $4 \times 10^{-4}$ (b) 0.02 (c) $2.5 \times 10^2$ (d) 50.0

The equilibrium constant $(\mathrm{K})$ for the reaction $\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NO}(\mathrm{g})$ at temperature T is $4 \times 10^{-4}$. The value of $\mathrm{K}_{\mathrm{c}}$ for the reaction, $\mathrm{NO}(\mathrm{g}) \rightarrow \frac{1}{2} \mathrm{~N}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g})$ at the same temperature is
[2012]
(a) $4 \times 10^{-4}$
(b) 0.02
(c) $2.5 \times 10^2$
(d) 50.0

Key Concepts

Equilibrium Constant

The equilibrium constant is a dimensionless value that quantifies the ratio of the concentrations (or partial pressures) of products to reactants at equilibrium at a given temperature. It encapsulates the position of equilibrium and is used to predict the extent to which a reaction will proceed.

Reversing a Reaction

When a chemical reaction is reversed, the equilibrium constant for the new reaction becomes the reciprocal of the original equilibrium constant. This is because the roles of reactants and products are exchanged, altering the ratio of their concentrations or partial pressures at equilibrium.

Manipulation of Reaction Stoichiometry

Changing the stoichiometric coefficients in a balanced chemical equation involves raising the equilibrium constant to a power that is equal to the factor by which the reaction is scaled. For example, if a reaction is halved, the equilibrium constant is taken to the power of one-half, reflecting the proportional change in the reaction’s expression.

Exponentiation of Equilibrium Constants

Exponentiation of the equilibrium constant occurs when the entire chemical equation is multiplied or divided by a factor. This mathematical property ensures the equilibrium constant correctly reflects the change in the reaction’s stoichiometry, maintaining the consistency of thermodynamic predictions.

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