6. A. Calculate the potential of the cell where the reaction: 2 HCIO2-→ HCIO + CIO3 + H*occurs if: [HCIO2] = 0.01 M; [HCIO] = 0.10 M; [CIO3¯] = 0.10 M and pH = 5.0%3D%3D%3DB. Taking all species to be 1 M except HCIO2, calculate the concentration of HCIO2 atwhich the reaction would no longer be spontaneous.

For this concentration cell, Potential of the cell will be, Ecell = -0.0591nlog Q where Q =…

6. A. Calculate the potential of the cell where the reaction: 2 HCIO - → HCIO + CIO3 + H* occurs if: [HCIO2] = 0.01 M; [HCIO] = 0.10 M; [CIO3¯] = 0.10 M and pH = 5.0 %3D %3D B. Taking all species to be 1 M except HCIO2, calculate the concentration of HCIO2 at which the reaction would no longer be spontaneous.

6. A. Calculate the potential of the cell where the reaction: 2 HCIO - → HCIO + CIO3 + H* occurs if: [HCIO2] = 0.01 M; [HCIO] = 0.10 M; [CIO3¯] = 0.10 M and pH = 5.0 %3D %3D B. Taking all species to be 1 M except HCIO2, calculate the concentration of HCIO2 at which the reaction would no longer be spontaneous.

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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