In $H_{2} - O_{2}$ fuel cell the reaction occuring at cathode is:

$2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (ℓ)$

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$O_{2} (g) + 2 H_{2} O (ℓ) + 4 e^{-} \to 4 O H^{-} (a q)$

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$H^{+} + e^{-} \to \frac{1}{2} H 2$

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$H^{+} (a q) + O H (a q) \to H_{2} O (ℓ)$

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Solution

The correct option is B
$O_{2} (g) + 2 H_{2} O (ℓ) + 4 e^{-} \to 4 O H^{-} (a q)$

$O_{2} (g) + 2 H_{2} O (ℓ) + 4 e^{-} \to 4 O H^{-} (a q)$

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Similar questions

In H₂ - O₂ fuel cell the reaction occuring at cathode is :

H_{2} - O_{2}

H_{2} - O_{2}

In $H_{2} - O_{2}$ fuel cell the reaction occuring at cathode is:

A fuel cell is:

I.A voltaic cell in which continuous supply of fuels are sent at anode to perform oxidation.

II. A voltaic cell in which fuels such as :

$C H_{4}, H_{2}$ and CO are used up at anode.

III. One which involves the reaction of $H_{2} O_{2}$ fuel cell such as:

Anode : $2 H_{2} + 4 ⊖ O H \to 4 H_{2} O (l) + 4 e^{-}$

Cathode : $O_{2} + 2 H_{2} O (l) + 4 e^{-} \to 4 ⊖ O H$

IV. The efficiency of $H_{2} - O_{2}$ fuel cell is $70$ to $75 %$ .

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