Phosphorus pentachloride decomposes to form phosphorus trichloride and chlorine according to the following equilibrium process:  PCl5(g) ⇌ PCl3(g) + Cl2(g) Kp=0.720 (at 250 °C) 0.200 atm PCl5, 0.750 atm PCl3, and 1.20 atm Cl2 are combined in a sealed flask at 250 °C and the reaction is allowed to reach equilibrium. Is the reaction considered reactant-favored, product-favored, or neither? In which direction will the reaction shift? Calculate the equilibrium partial pressure of PCl5PCl5 in the reaction mixture. Calculate the equilibrium partial pressure of Cl2Cl2 in the reaction mixture.

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