The equilibrium constant, K, for the following reaction is 1.20x10-2at 500 K.PCI5(g) PCI3(g) + Cl2(g)An equilibrium mixture of the three gases in a 1.00 L flask at 500 Kcontains 0.274 M PCI5, 5.73x102 M PCl, and 5.73x102 M Cl,.What will be the concentrations of the three gases once equilibriumhas been reestablished, if 4.44x10-² mol of Cl(g) is added to theflask?[PCI5] =%3D[PCI3] =%3D[Ch]%3DMMM

The equilibrium constant K for the reaction would be, K = [PCl3][Cl2]/[PCl5] let x be the change in…

An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.274 M PCI5, 5.73x10² M PCI3 and 5.73x102 M Cl. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.44x10² mol of Cl2(g) is added to the flask?

An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.274 M PCI5, 5.73x10² M PCI3 and 5.73x102 M Cl. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.44x10² mol of Cl2(g) is added to the flask?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

100%

The equilibrium constant, K, for the following reaction is 1.20x10-2
at 500 K.
PCI5(g) PCI3(g) + Cl2(g)
An equilibrium mixture of the three gases in a 1.00 L flask at 500 K
contains 0.274 M PCI5, 5.73x102 M PCl, and 5.73x102 M Cl,.
What will be the concentrations of the three gases once equilibrium
has been reestablished, if 4.44x10-² mol of Cl(g) is added to the
flask?
[PCI5] =
%3D
[PCI3] =
%3D
[Ch]
%3D
MMM

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