Answer:
Option B
Explanation:
In a hydrogen-oxygen fuel cell, following reactions take place to create a potential difference between the two electrodes.
$2H_{2} (g) + 4OH^{-}(aq) \rightarrow 4H2O (l) + 4e^{-}$
$O_{2} (g) + 2H_{2}O(l) + 4e^{-} \rightarrow 4OH^{-}(aq)$
$Overall reaction = 2H_{2} (g) + O_{2} (g) \rightarrow 2H_{2}O(l)$
the net reaction is the same as burning (combustion) of hydrogen to form water.
