AP Chemistry
7.7 Calculating Equilibrium Concentrations
7.4 Calculating the Equilibrium Constant
A \(1.2\text{ mol}\) sample of \(\text{NOCl(g)}\) is placed into a previously evacuated, rigid \(2.0\text{ L}\) container and heated to \(500\text{ K}\). The system reaches equilibrium according to the equation below.
\[ 2\text{NOCl(g)} \rightleftharpoons 2\text{NO(g)} + \text{Cl}_2\text{(g)} \]
At equilibrium, analysis shows that \(0.40\text{ mol}\) of \(\text{Cl}_2\text{(g)}\) is present in the container. Based on these data, what is the value of the equilibrium constant, \(K_c\), for the reaction at \(500\text{ K}\)?
\[ 2\text{NOCl(g)} \rightleftharpoons 2\text{NO(g)} + \text{Cl}_2\text{(g)} \]
At equilibrium, analysis shows that \(0.40\text{ mol}\) of \(\text{Cl}_2\text{(g)}\) is present in the container. Based on these data, what is the value of the equilibrium constant, \(K_c\), for the reaction at \(500\text{ K}\)?
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