Chapter 8, Problem 8.46E

A sample of gaseous $\text{BrCl}$ is allowed to decompose in a closed container at $25°\text{C}$:

$\text{2BrCl}\left(\text{g}\right)\rightleftarrows {\text{Br}}_2\left(\text{g}\right)+{\text{Cl}}_{\text{2}}\left(\text{g}\right)$

When the reaction reaches equilibrium, the following concentrations are measured: $\left[\text{BrCl}\right]=0.38\text{M}$, $\left[{\text{Cl}}_2\right]=0.26\text{M}$, $\left[{\text{Br}}_2\right]=0.26\text{M}$. Evaluate the equilibrium constant for the reaction at $25°\text{C}$.