For the reaction equilibrium, [2003] N2 O4( g) ⇌2 NO(g) the concentrations of N2 O4 and NO2 at e

step 1 In this problem, for the reaction equilibrium, N204 reacts reversively to give 2 moles of NO2 ga

For the reaction equilibrium, [2003] N2 O4( g) ⇌2 NO(g) the...

For the reaction equilibrium, [2003] $\mathrm{N}_2 \mathrm{O}_4(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})$ the concentrations of $\mathrm{N}_2 \mathrm{O}_4$ and $\mathrm{NO}_2$ at equilibrium are $4.8 \times 10^{-2}$ and $1.2 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1}$ respectively. The value of $K_c$ for the reaction is (a) $3.3 \times 10^2 \mathrm{~mol} \mathrm{~L}^{-1}$ (b) $3 \times 10^{-1} \mathrm{~mol} \mathrm{~L}^{-1}$ (c) $3 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1}$ (d) $3 \times 10^3 \mathrm{~mol} \mathrm{~L}^{-1}$

For the reaction equilibrium,
[2003]
$\mathrm{N}_2 \mathrm{O}_4(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})$
the concentrations of $\mathrm{N}_2 \mathrm{O}_4$ and $\mathrm{NO}_2$ at equilibrium are $4.8 \times 10^{-2}$ and $1.2 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1}$ respectively. The value of $K_c$ for the reaction is
(a) $3.3 \times 10^2 \mathrm{~mol} \mathrm{~L}^{-1}$
(b) $3 \times 10^{-1} \mathrm{~mol} \mathrm{~L}^{-1}$
(c) $3 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1}$
(d) $3 \times 10^3 \mathrm{~mol} \mathrm{~L}^{-1}$

Key Concepts

Reaction Stoichiometry

Reaction stoichiometry refers to the quantitative relationships between reactants and products in a chemical reaction, as specified by the coefficients in a balanced equation. These coefficients determine the exponents in the equilibrium constant expression, thereby influencing how changes in the concentration of one species affect the overall equilibrium state.

Unit Analysis in Equilibrium Calculations

Unit analysis is essential in equilibrium calculations, ensuring that concentration measurements (typically in mol L?¹) are correctly manipulated to provide consistent and meaningful values for the equilibrium constant. Proper handling of units helps confirm that the calculated value of Kc reflects the correct relationship between reactants and products.

Equilibrium Constant (Kc)

The equilibrium constant, Kc, quantifies the ratio of concentrations of products to reactants for a reaction at equilibrium, with each concentration raised to an exponent equal to its stoichiometric coefficient. It serves as a key indicator of the extent to which a reaction proceeds under equilibrium conditions.

Law of Mass Action

The Law of Mass Action provides the foundation for writing the equilibrium expression. It states that at equilibrium, the rate of the forward reaction equals that of the reverse reaction, and the equilibrium constant is defined by the product of the concentrations of the products, each raised to their respective reaction coefficients, divided by the product of the concentrations of the reactants, raised to their corresponding coefficients.

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