Consider a fuel cell that uses methane ("natural gas") as fuel. The reaction is                         CH4 + 2O2 → 2H2O +CO2 Assuming ideal performance, how much electrical work can you get out of the cell, for each mole of methane fuel?

Principles of Modern Chemistry
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Chapter17: Electrochemistry
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Consider a fuel cell that uses methane ("natural gas") as fuel. The reaction is

                        CH4 + 2O2 → 2H2O +CO2

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

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