Calculating equilibrium concentrations when the net reaction proceeds forward Consider mixture B, which will cause the net reaction to proceed forward. Concentration (M)initial:change:equilibrium:[XY]0.500−x0.500−xnet→⇌[X]0.100+x0.100+x+[Y]0.100+x0.100+xnet→Concentration (M)[XY]⇌[X]+[Y]initial:0.5000.1000.100change:−x+x+xequilibrium:0.500−x0.100+x0.100+x The change in concentration, xxx, is negative for the reactants because they are consumed and positive for the products because they are produced. Part A Based on a KcKcK_c value of 0.170 and the given data table, what are the equilibrium concentrations of XYXY, XX, and YY, respectively? Express the molar concentrations numerically. ........................................................................................................................ Calculating equilibrium concentrations when the net reaction proceeds in reverse Consider mixture C, which will cause the net reaction to proceed in reverse. Concentration (M)initial:change:equilibrium:[XY]0.200+x0.200+x←net⇌[X]0.300−x0.300−x+[Y]0.300−x0.300−x←netConcentration (M)[XY]⇌[X]+[Y]initial:0.2000.3000.300change:+x−x−xequilibrium:0.200+x0.300−x0.300−x The change in concentration, xxx, is positive for the reactants because they are produced and negative for the products because they are consumed. Part B Based on a KcKcK_c value of 0.170 and the data table given, what are the equilibrium concentrations of XYXY, XX, and YY, respectively? Express the molar concentrations numerically.

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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Calculating equilibrium concentrations when the net reaction proceeds forward

Consider mixture B, which will cause the net reaction to proceed forward.

Concentration (M)initial:change:equilibrium:[XY]0.500−x0.500−xnet→⇌[X]0.100+x0.100+x+[Y]0.100+x0.100+xnet→Concentration (M)[XY]⇌[X]+[Y]initial:0.5000.1000.100change:−x+x+xequilibrium:0.500−x0.100+x0.100+x

The change in concentration, xxx, is negative for the reactants because they are consumed and positive for the products because they are produced.

Part A

Based on a KcKcK_c value of 0.170 and the given data table, what are the equilibrium concentrations of XYXY, XX, and YY, respectively?

Express the molar concentrations numerically.

........................................................................................................................

Calculating equilibrium concentrations when the net reaction proceeds in reverse

Consider mixture C, which will cause the net reaction to proceed in reverse.

Concentration (M)initial:change:equilibrium:[XY]0.200+x0.200+x←net⇌[X]0.300−x0.300−x+[Y]0.300−x0.300−x←netConcentration (M)[XY]⇌[X]+[Y]initial:0.2000.3000.300change:+x−x−xequilibrium:0.200+x0.300−x0.300−x

The change in concentration, xxx, is positive for the reactants because they are produced and negative for the products because they are consumed.

Part B

Based on a KcKcK_c value of 0.170 and the data table given, what are the equilibrium concentrations of XYXY, XX, and YY, respectively?

Express the molar concentrations numerically.

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