The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K.PCl5(g)=PCl3(g)+Cl2(g)An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.164 M PCl5, 4.43×10-2 M PCl3 and 4.43×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 2.27×10-2 mol of Cl2(g) is added to the flask?[PCl5]=______ M[PCl3]= ______M[Cl2]=______ M

Equilibrium is a state of the chemical reaction at which the rate of forward reaction becomes equal…

Answered: The equilibrium constant, K, for the…

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section: Chapter Questions

Problem 16PS: The equilibrium constant, Kc, for the reaction N2O4(g) 2 NO2(g) at 25 C is 5.9 103. Suppose 15.6 g...

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The equilibrium constant, K, for the following reaction is 1.20×10^-2 at 500 K.

PCl5(g)=PCl3(g)+Cl2(g)

An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.164 M PCl₅, 4.43×10^-2 M PCl₃ and 4.43×10^-2 M Cl₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if 2.27×10^-2 mol of Cl₂(g) is added to the flask?

[PCl₅]	=	______ M
[PCl₃]	=	______M
[Cl₂]	=	______ M

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