In a hydrogen-oxygen fuel cell, combustion of hydrogen occurs to

A
generate heat
B
create potential difference between the two electrodes
C
produce high purity water
D
remove adsorbed oxygen from electrode surface.

Solution:

The reaction occuring in hydrogen-oxygen fuel all are

At anode $2 H_{2} (g) + 4 {OH}^{-} (aq) \to 4 H_{2} O (l) + 4 e^{-}$

At cathode $O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 {OH}^{-} (aq)$

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

The net reaction is the oxidation of $H_{2} (g)$ . There exists potential difference between anode and cathode. This creates a potential difference between the two terminals.

Solution:

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