In the equation below, which species acts as the oxidizing agent?
$Pb (s) + {PbO}_{2} (s) + 2 H^{+} (a q) + 2 {HSO}_{4}^{-} (a q)$ $⟶ 2 {PbSO}_{4} (s) + 2 H_{2} O (l)$

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${PbO}_{2} (s)$

${HSO}_{4}^{-} (a q)$

$H^{+} (a q)$

$Pb (s)$

answer is B.

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Detailed Solution

In the equation below, ${PbO}_{2} (s)$ species acts as the oxidizing agent.

$Pb (s) + {PbO}_{2} (s) + 2 H^{+} (a q) + 2 {HSO}_{4}^{-} (a q)$ $⟶ 2 {PbSO}_{4} (s) + 2 H_{2} O (l)$

$Pb$ is oxidized, ad ${PbO}_{2}$ is reduced.
${PbO}_{2}$ is oxidizing agent and $Pb$ is reducing agent.

Hence, option B is correct.

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