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Consider a fuel cell that uses methane (“natural gas”) as

An Introduction to Thermal Physics | 1st Edition | ISBN: 9780201380279 | Authors: Daniel V. Schroeder ISBN: 9780201380279 40

Solution for problem 5P Chapter 5

An Introduction to Thermal Physics | 1st Edition

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An Introduction to Thermal Physics | 1st Edition | ISBN: 9780201380279 | Authors: Daniel V. Schroeder

An Introduction to Thermal Physics | 1st Edition

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Problem 5P Problem 5P

Consider a fuel cell that uses methane (“natural gas”) as fuel. The reaction is

CH4 + 2O2 → 2H2O + CO2

(a) Use the data at the back of this book to determine the values of ΔH and ΔG for this reaction, for one mole of methane. Assume that the reaction takes place at room temperature and atmospheric pressure.

(b) Assuming ideal performance, how much electrical work can you get out of the cell, for each mole of methane fuel?

(c) How much waste heat is produced, for each mole of methane fuel?

(d) The steps of this reaction are

at – electrode: CH4 + 2H2O → CO2 + 8H+ + 8e–;

at + electrode: 2O2 + 8H+ + 8e– → 4H2O.

What is the voltage of the cell?

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Textbook: An Introduction to Thermal Physics
Edition: 1
Author: Daniel V. Schroeder
ISBN: 9780201380279

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