AP Chemistry
7.4 Calculating the Equilibrium Constant
7.3 Reaction Quotient and Equilibrium Constant
A sample of \(\text{PCl}_5\text{(g)}\) is placed in a rigid, sealed container and heated to a constant temperature. The system reaches equilibrium according to the following equation:
\[ \text{PCl}_5\text{(g)} \rightleftharpoons \text{PCl}_3\text{(g)} + \text{Cl}_2\text{(g)} \]
At equilibrium, the molar concentrations of the gases are measured to be \([\text{PCl}_5] = 0.40 \text{ M}\), \([\text{PCl}_3] = 0.20 \text{ M}\), and \([\text{Cl}_2] = 0.30 \text{ M}\). What is the value of the equilibrium constant, \(K_c\), for the reaction at this temperature?
\[ \text{PCl}_5\text{(g)} \rightleftharpoons \text{PCl}_3\text{(g)} + \text{Cl}_2\text{(g)} \]
At equilibrium, the molar concentrations of the gases are measured to be \([\text{PCl}_5] = 0.40 \text{ M}\), \([\text{PCl}_3] = 0.20 \text{ M}\), and \([\text{Cl}_2] = 0.30 \text{ M}\). What is the value of the equilibrium constant, \(K_c\), for the reaction at this temperature?
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