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 ?