CS 2( g) + 3Cl 2( g) <=> CCl 4( g) + S 2Cl 2( g) At a given temperature, the reaction above is at equilibrium when [CS2] = 0.075 M, [Cl2] = 0.35 M, [CCl4] = 0.25 M, and [S2Cl2] = 0.45 M. What will be the direction of the reaction when the reactants and products have the following concentrations: CS2 = 0.15 M, Cl2 = 0.15 M, CCl4 = 0.45M, and S2Cl2 = 0.31 M? I would like help with this problem I am solving for Kc and then Qc I believe.
CS 2( g) + 3Cl 2( g) <=> CCl 4( g) + S 2Cl 2( g) At a given temperature, the reaction above is at equilibrium when [CS2] = 0.075 M, [Cl2] = 0.35 M, [CCl4] = 0.25 M, and [S2Cl2] = 0.45 M. What will be the direction of the reaction when the reactants and products have the following concentrations: CS2 = 0.15 M, Cl2 = 0.15 M, CCl4 = 0.45M, and S2Cl2 = 0.31 M? I would like help with this problem I am solving for Kc and then Qc I believe.
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 3RQ
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- CS 2( g) + 3Cl 2( g) <=> CCl 4( g) + S 2Cl 2( g)
At a given temperature, the reaction above is at equilibrium when [CS2] = 0.075 M, [Cl2] = 0.35 M, [CCl4] = 0.25 M, and [S2Cl2] = 0.45 M. What will be the direction of the reaction when the reactants and products have the following concentrations: CS2 = 0.15 M, Cl2 = 0.15 M, CCl4 = 0.45M, and S2Cl2 = 0.31 M?
I would like help with this problem I am solving for Kc and then Qc I believe.
for Kc I set up the following equation using the molarity values in the brackets as (.25)(.45)/(.075)(.035)^3 and the Qc as (.45)(.31)/(.15)(.15)^3
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