AP Chemistry
7.7 Calculating Equilibrium Concentrations
A \(1.0 \text{ L}\) rigid reaction vessel is filled with \(1.0 \text{ mol}\) of \(\text{NOCl}(g)\) at a fixed temperature. The reaction proceeds according to the equation below.
\[ 2\,\text{NOCl}(g) \rightleftharpoons 2\,\text{NO}(g) + \text{Cl}_2(g) \]
At this temperature, \(K_c = 3.2 \times 10^{-8}\). Based on an ICE table and assuming that the change in concentration of \(\text{NOCl}(g)\) is negligible, what is the equilibrium concentration of \(\text{Cl}_2(g)\)?
\[ 2\,\text{NOCl}(g) \rightleftharpoons 2\,\text{NO}(g) + \text{Cl}_2(g) \]
At this temperature, \(K_c = 3.2 \times 10^{-8}\). Based on an ICE table and assuming that the change in concentration of \(\text{NOCl}(g)\) is negligible, what is the equilibrium concentration of \(\text{Cl}_2(g)\)?
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