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An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr,...

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Chemistry

An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) haspartial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr,respectively. A quantity of Cl2(g) is injected into the mixture,and the total pressure jumps to 263.0 Torr (at the moment ofmixing). The system then re-equilibrates. The appropriate chemicalequation is

PCl3(g) + Cl2(g) <---> PCl5(g)

Calculate the new partial pressures after equilibrium isreestablished.

P PCl3 = ? torr

P PCl2 = ? torr

P PCl5 = ? torr

Answer & Explanation Solved by verified expert
3.6 Ratings (641 Votes)
pPCl3 680 torr pCl2 264 torr pPCl5 2234 torr Explanation pressure equilibrium constant Kp pPCl5eq pPCl3eqpCl2eq Kp 2170 torr 132 torr 132 torr Kp 12454 Total pressure    See Answer
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