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The U.S. space program has supported extensive research to developfuel cells. The early space missions used a fuel cell based on thereaction of hydrogen and oxygen to form water :

2H₂(g) + O₂(g) → 2H₂O(l)

The half-reactions for this cell are :

anode; 2H₂ + 4OH^- → 4H₂O +4e^-

cathode: 4e^- + O₂ + 2H₂O → 4OH^-

If this cell is to produce a current of 11.0 A for 105.0 hours, what mass in grams of hydrogen gas would need to be available ?

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Category:- Chemistry
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