Which of the following species acts as reducing agent during working of hydrogen-oxygen fuel cell?

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In a hydrogen-oxygen fuel cell, the reactions at the electrodes are:

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

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

Since $H_{2}$ undergoes oxidation by losing electrons, it acts as the reducing agent. $O_{2}$ undergoes reduction and acts as the oxidizing agent.

Answer: $H_{2}$

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