Chapter 15, Problem 83AP

Consider the following reaction at $\text{1600°C:}$

$\text{B}{\text{r}}_{\text{2}}\text{(}g\text{)}\underset{}{\rightleftarrows }\text{2Br(}g\text{)}$

When 1.05 moles of ${\text{Br}}_{\text{2}}$ are put in a 0.980-L flask. 1.20 percent of the ${\text{Br}}_{\text{2}}$ undergoes dissociation. Calculate the equilibrium constant K_c for the reaction.