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In a hydrogen oxyge fuel cell, electrici...

In a hydrogen oxyge fuel cell, electricity is produced. In this process `H_2`(g) is oxided at anode and `O_2`(g) reduced at cathode
Given: Cathode `O_2(g)+2H_2O(l)+4e^(-)to4OH^(-)(aq)`
Anode `H_2(g)+2OH^(-)(aq)to2H_2O(l)+2e^(-)`
4.48 litre `H_2` at 1atm and 273 k oxidised in 9650 sec.
The current produced is (in amp):

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In a hydrogen oxyge fuel cell, electricity is produced. In this process H_2 (g) is oxided at anode and O_2 (g) reduced at cathode Given: Cathode O_2(g)+2H_2O(l)+4e^(-)to4OH^(-)(aq) Anode H_2(g)+2OH^(-)(aq)to2H_2O(l)+2e^(-) 4.48 litre H_2 at 1atm and 273 k oxidised in 9650 sec. The mass of water produced is :

In a hydrogen oxyge fuel cell, electricity is produced. In this process H_2 (g) is oxided at anode and O_2 (g) reduced at cathode Given: Cathode O_2(g)+2H_2O(l)+4e^(-)to4OH^(-)(aq) Anode H_2(g)+2OH^(-)(aq)to2H_2O(l)+2e^(-) 4.48 litre H_2 at 1atm and 273 k oxidised in 9650 sec. The mass of water produced is :

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Write anode and cathode reactions of H_2-O_2 fuel cell.

Which of the following will give H_2(g) at cathode and O_2(g) at anode on electrolysis using platinum electrodes?