AP Chemistry
7.6 Properties of the Equilibrium Constant
The equilibrium constants for three reactions at a constant temperature of \(1000\text{ K}\) are given below.
\[\text{H}_2(g) + \dfrac{1}{2}\,\text{S}_2(g) \rightleftharpoons \text{H}_2\text{S}(g) \quad K_1 = 5.0 \times 10^{-2}\]
\[\text{SO}_2(g) \rightleftharpoons \dfrac{1}{2}\,\text{S}_2(g) + \text{O}_2(g) \quad K_2 = 2.0 \times 10^{-3}\]
\[2\,\text{H}_2(g) + \text{O}_2(g) \rightleftharpoons 2\,\text{H}_2\text{O}(g) \quad K_3 = 5.0 \times 10^{-4}\]
Based on this information, what is the value of the equilibrium constant, \(K\), for the reaction \(2\,\text{H}_2\text{S}(g) + 3\,\text{O}_2(g) \rightleftharpoons 2\,\text{SO}_2(g) + 2\,\text{H}_2\text{O}(g)\) at \(1000\text{ K}\)?
\[\text{H}_2(g) + \dfrac{1}{2}\,\text{S}_2(g) \rightleftharpoons \text{H}_2\text{S}(g) \quad K_1 = 5.0 \times 10^{-2}\]
\[\text{SO}_2(g) \rightleftharpoons \dfrac{1}{2}\,\text{S}_2(g) + \text{O}_2(g) \quad K_2 = 2.0 \times 10^{-3}\]
\[2\,\text{H}_2(g) + \text{O}_2(g) \rightleftharpoons 2\,\text{H}_2\text{O}(g) \quad K_3 = 5.0 \times 10^{-4}\]
Based on this information, what is the value of the equilibrium constant, \(K\), for the reaction \(2\,\text{H}_2\text{S}(g) + 3\,\text{O}_2(g) \rightleftharpoons 2\,\text{SO}_2(g) + 2\,\text{H}_2\text{O}(g)\) at \(1000\text{ K}\)?
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