In a hydrogen oxygen fuel cell, electricity is produced. In this process H2(g) is oxidised at anode and O2(g) reduced at cathode. Given : Cathode: O2(g)+2H2O(l)+4e−→4OH−(aq) Anode : H2(g)+2OH−(aq)→2H2O(l)+2e− 4.48 L of H2 at 1 atm and 273 K is oxidised in 9650 sec.
The mass of water produced is (in grams):