Use the equilibrium constants for the following reactions
$\begin{array}{ll}2 \mathrm{NO}(g) \rightleftharpoons \mathrm{N}_{2}(g) +\mathrm{O}_{2}(g) & K_{1}=2.4 \times 10^{30} \\2 \mathrm{NO}(g) +\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g) & K_{2}=2.4 \times 10^{12}\end{array}$
To determine the equilibrium constant for the reaction below.
N₂(g) + 2O₂(g) ⇌ 2NO₂(g)

Question

Use the equilibrium constants for the following reactions

\begin{array}{ll}2 \mathrm{NO}(g) \rightleftharpoons \mathrm{N}_{2}(g) +\mathrm{O}_{2}(g) & K_{1}=2.4 \times 10^{30} \\2 \mathrm{NO}(g) +\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g) & K_{2}=2.4 \times 10^{12}\end{array}

To determine the equilibrium constant for the reaction below.
N₂(g) + 2O₂(g) ⇌ 2NO₂(g)

Quizplus · Accepted Answer

To find the equilibrium constant for the reaction $ \mathrm{N}_{2}(g) + 2\mathrm{O}_{2}(g) \rightleftharpoons 2\mathrm{NO}_{2}(g) $, we need to combine the given reactions. The first reaction is reversed and halved, and the second reaction is used as is. The equilibrium constant for the desired reaction is $ K = \frac{K_2}{K_1} = \frac{2.4 \times 10^{12}}{2.4 \times 10^{30}} = 1.0 \times 10^{-18} $.

Use the Equilibrium Constants for the Following Reactions To Determine the Equilibrium Constant for the Reaction Below