An equilibrium mixture of PCI, (g), PCl, (g), and Cl, (g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Tor,respectively. A quantity of Cl, (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 chemical equation for this reaction isPCI, (g) + Cl, (g) = PCI, (g)Calculate the new partial pressures, P, after equilibrium is reestablished.TorrPPCI, =TorrPCl2TorrPpCl,II

PCl3 Cl2 PCl5 Initial 13.2 13.2 217 Change +x +x -x Equilibrium 13.2+x 13.2+x 217-x *…

Answered: Calculate the new partial pressures, P,…

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Calculate the new partial pressures, P, after equilibrium is reestablished.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 33P

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Question

An equilibrium mixture of PCI, (g), PCl, (g), and Cl, (g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Tor,
respectively. A quantity of Cl, (g) is injected into the mixture, and the total pressure jumps to 263.0 Torr at the moment of
mixing. The system then re-equilibrates.
The chemical equation for this reaction is
PCI, (g) + Cl, (g) = PCI, (g)
Calculate the new partial pressures, P, after equilibrium is reestablished.
Torr
PPCI, =
Torr
PCl2
Torr
PpCl,
II

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