Based on these raw experimental data, calculate the Faraday constant.V(H2) = 41.1 ml; V(02) = 19.5 ml%3DP atm = 760.5 mmHgTemperature = 27 °CTime of electrolysis: 46 min - 2769 secondsCurrent, i= 0.108 mA.

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Based on these raw experimental data, calculate the Faraday constant. V(H2) = 41.1 ml; V(02) = 19.5 ml %3! P atm = 760.5 mmHg %3D Temperature = 27 °C Time of electrolysis: 46 min = 2769 seconds Current, i= 0.108 mA.

Based on these raw experimental data, calculate the Faraday constant. V(H2) = 41.1 ml; V(02) = 19.5 ml %3! P atm = 760.5 mmHg %3D Temperature = 27 °C Time of electrolysis: 46 min = 2769 seconds Current, i= 0.108 mA.

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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Question

Based on these raw experimental data, calculate the Faraday constant.
V(H2) = 41.1 ml; V(02) = 19.5 ml
%3D
P atm = 760.5 mmHg
Temperature = 27 °C
Time of electrolysis: 46 min - 2769 seconds
Current, i= 0.108 mA.

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