AP Chemistry
7.6 Properties of the Equilibrium Constant
Two gas-phase equilibria and their equilibrium constants at \(298\text{ K}\) are shown below.
\[2\text{NO}(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}_2(g) \quad K_1 = 1.6 \times 10^5\]
\[\text{N}_2\text{O}_4(g) \rightleftharpoons 2\text{NO}_2(g) \quad K_2 = 4.0 \times 10^{-4}\]
What is the value of the equilibrium constant, \(K\), for the reaction below at \(298\text{ K}\)?
\[\text{NO}(g) + \dfrac{1}{2}\text{O}_2(g) \rightleftharpoons \dfrac{1}{2}\text{N}_2\text{O}_4(g)\]
\[2\text{NO}(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}_2(g) \quad K_1 = 1.6 \times 10^5\]
\[\text{N}_2\text{O}_4(g) \rightleftharpoons 2\text{NO}_2(g) \quad K_2 = 4.0 \times 10^{-4}\]
What is the value of the equilibrium constant, \(K\), for the reaction below at \(298\text{ K}\)?
\[\text{NO}(g) + \dfrac{1}{2}\text{O}_2(g) \rightleftharpoons \dfrac{1}{2}\text{N}_2\text{O}_4(g)\]
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