Tutored Practice Problem 16.3.2
Use an ICE table to calculate K.
A mixture of CO and $Cl_2$ is allowed to react at 567 K.
$CO(g) + Cl_2(g) \rightleftharpoons COCl_2(g)$
The initial concentration of the reactants are $[CO] = 0.4380$ M and $[Cl_2] = 0.4590$ M. After the system reaches equilibrium, it is found that the $Cl_2$ concentration has decreased to 0.0514 M. Based on these data, determine the value of the equilibrium constant, K, for this reaction.
K =