Phosphorus pentachloride gas, PCl5(g), will decompose to phosphorus trichloride, PCl3(g), and chlorine, Cl2(g), at 160⁰C. In a sealed vessel, the reaction will proceed to equilibrium: PCl5(g) ↔ PCl3(g) + Cl2(g) A chemist places 3.00 mol of phosphorus pentachloride gas into a sealed 1.50 L flask at 160⁰C. At equilibrium, he observes there is 0.300 mol of phosphorus trichloride gas and some chlorine gas. Calculate the equilibrium concentrations of gaseous phosphorus pentachloride and chlorine gas.
