AP Chemistry
7.4 Calculating the Equilibrium Constant
7.3 Reaction Quotient and Equilibrium Constant
A sample of \(\text{NOCl(g)}\) is placed into a rigid, evacuated \(2.0\text{ L}\) container and heated until equilibrium is reached at \(350^\circ\text{C}\) according to the following equation:
\[ 2\text{NOCl(g)} \rightleftharpoons 2\text{NO(g)} + \text{Cl}_2\text{(g)} \]
At equilibrium, the mixture contains \(0.40\text{ mol}\) of \(\text{NOCl(g)}\), \(0.10\text{ mol}\) of \(\text{NO(g)}\), and \(0.080\text{ mol}\) of \(\text{Cl}_2\text{(g)}\). What is the value of the equilibrium constant, \(K_c\), for the reaction at this temperature?
\[ 2\text{NOCl(g)} \rightleftharpoons 2\text{NO(g)} + \text{Cl}_2\text{(g)} \]
At equilibrium, the mixture contains \(0.40\text{ mol}\) of \(\text{NOCl(g)}\), \(0.10\text{ mol}\) of \(\text{NO(g)}\), and \(0.080\text{ mol}\) of \(\text{Cl}_2\text{(g)}\). What is the value of the equilibrium constant, \(K_c\), for the reaction at this temperature?
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