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):

In a hydrogen oxygen fuel cell, electricity is produced. In this proce

1.	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):
Answer» In a hydrogen oxygen fuel cell, electricity is produced. In this process $H_{2} (g)$ is oxidised at anode and $O_{2} (g)$ reduced at cathode. Given : Cathode: $O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)$ Anode : $H_{2} (g) + 2 O H^{-} (a q) \to 2 H_{2} O (l) + 2 e^{-}$ $4.48 L$ of $H_{2}$ at $1 atm$ and $273 K$ is oxidised in $9650 sec$ . The mass of water produced is (in grams):