1. A voltaic cell consists of two half-cells. One of the half-cells contains a platinum electrode surrounded by chromium (I) and dichromate ions. The other half-cell contains a platinum electrode surrounded by bromate ions and liquid bromine. Assume that the cell reaction, which produces a positive voltage, involves both chromium (III) and bromate ions. The cell is at 25°C. Information for the bromate reduction half reaction is as follows: 2B1O,-(ag) + 12H*(aq) + 10e- Br2(1) + 6H,0 Ered = 1.478 V (a) Write the cell diagram notation (b) Calculate E* for the cell (c) Calculate the voltage of the cell when all ionic species except H+ are 0.1500M and the pH is at -0.301.

1. A voltaic cell consists of two half-cells. One of the half-cells contains a platinum electrode surrounded by chromium (I) and dichromate ions. The other half-cell contains a platinum electrode surrounded by bromate ions and liquid bromine. Assume that the cell reaction, which produces a positive voltage, involves both chromium (III) and bromate ions. The cell is at 25°C. Information for the bromate reduction half reaction is as follows: 2B1O,-(ag) + 12H(aq) + 10e- Br2(1) + 6H,0 Ered = 1.478 V (a) Write the cell diagram notation (b) Calculate E for the cell (c) Calculate the voltage of the cell when all ionic species except H+ are 0.1500M and the pH is at -0.301.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

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