(Solved): Consider the reaction: CCl4(s)C(s)+2Cl2(s) At equilibrium at constant temperature, the ...

Consider the reaction: ${\mathrm{CCl}}_4(\mathrm{s})?\mathrm{C}(s)+2{\mathrm{Cl}}_2(\mathrm{s})$ At equilibrium at constant temperature, the following quantities were measured: $\begin{array}{l}{P}_{\text{CCl m }}=3.7\text{ barr }\\ P_{{\mathrm{Cl}}_{\mathrm{m}}}=14\text{ barr }\\ \text{ mass }\mathrm{C}(\mathrm{s})=14\mathrm{g}\end{array}$ Calculate the pressure equilibrium constant, $K_p$, for this reaction at this temperature. Note: You do not need to convert any units because the reference state for gasses in the $K_p$ expression is defined as 1 barr. That is, the activity for a gas in $K_0$ is: $a_x=\frac{P_2}{1\text{ liar }}$ Report your answer to two significant figures. Example: 10