Hydrogen fuel cells produce electricity by utilizing a redox reaction between hydrogen gas and oxygen gas without the need for combustion. Oxidation of hydrogen gas to water happens at the anode, while reduction of oxygen gas to hydroxide happens at the cathode. A certain hydrogen fuel cell consumes pure hydrogen at the anode side at 80 kPa and uses air at 1 bar as the oxygen source in the cathode side. This fuel cell operates at 30 °C. Assuming no side reactions due to the existence of nitrogen in the cathode. a. Solve for the standard cell potential, E' cell b. Solve for the actual cell potential, Eeit c. What is the overall reaction? How is the overall reaction it different from hydrogen combustion?

Hydrogen fuel cells produce electricity by utilizing a redox reaction between hydrogen gas and oxygen gas without the need for combustion. Oxidation of hydrogen gas to water happens at the anode, while reduction of oxygen gas to hydroxide happens at the cathode. A certain hydrogen fuel cell consumes pure hydrogen at the anode side at 80 kPa and uses air at 1 bar as the oxygen source in the cathode side. This fuel cell operates at 30 °C. Assuming no side reactions due to the existence of nitrogen in the cathode. a. Solve for the standard cell potential, E' cell b. Solve for the actual cell potential, Eeit c. What is the overall reaction? How is the overall reaction it different from hydrogen combustion?

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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