AP Chemistry
7.6 Properties of the Equilibrium Constant
At a constant temperature \(T\), the equilibrium constants for the following reactions are given:
\[ \begin{aligned} 2\,\text{NO}_2\text{(g)} &\rightleftharpoons 2\,\text{NO(g)} + \text{O}_2\text{(g)} \quad &K_1 = 4.0 \times 10^{-4} \\ \text{N}_2\text{O(g)} + \text{NO}_2\text{(g)} &\rightleftharpoons 3\,\text{NO(g)} \quad &K_2 = 6.0 \times 10^{-2} \end{aligned} \]
Based on this information, what is the value of the equilibrium constant, \(K_c\), for the reaction represented below at the same temperature?
\[ 2\,\text{N}_2\text{O(g)} + \text{O}_2\text{(g)} \rightleftharpoons 4\,\text{NO(g)} \]
\[ \begin{aligned} 2\,\text{NO}_2\text{(g)} &\rightleftharpoons 2\,\text{NO(g)} + \text{O}_2\text{(g)} \quad &K_1 = 4.0 \times 10^{-4} \\ \text{N}_2\text{O(g)} + \text{NO}_2\text{(g)} &\rightleftharpoons 3\,\text{NO(g)} \quad &K_2 = 6.0 \times 10^{-2} \end{aligned} \]
Based on this information, what is the value of the equilibrium constant, \(K_c\), for the reaction represented below at the same temperature?
\[ 2\,\text{N}_2\text{O(g)} + \text{O}_2\text{(g)} \rightleftharpoons 4\,\text{NO(g)} \]
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