Consider the reaction: $\mathrm{H}_{2}…

Consider the reaction:
$\mathrm{H}_{2} \mathrm{SO}_{3}(\mathrm{aq})+\mathrm{Sn}^{4+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) ightarrow \mathrm{Sn}^{2+}(\mathrm{aq})+\mathrm{HSO}_{4}^{-}(\mathrm{aq})+3 \mathrm{H}^{+}(\mathrm{aq})$
Which of the following statements is correct?
  1. $\mathrm{Sn}^{4+}$ is the oxidizing agent because it undergoes oxidation
  2. $\mathrm{Sn}^{4+}$ is the reducing agent because it undergoes oxidation
  3. $\mathrm{H}_{2} \mathrm{SO}_{3}$ is the reducing agent because it undergoes oxidation
  4. $\mathrm{H}_{2} \mathrm{SO}_{3}$ is the reducing agent because it undergoes reduction

Solution

$\mathrm{H}_{2} \mathrm{SO}_{3}(\mathrm{aq})+\mathrm{Sn}^{4+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \underset{+6}{\longrightarrow} \mathrm{Sn}^{2+}(\mathrm{aq})+\mathrm{HSO}_{4}^{-}(\mathrm{aq})+3 \mathrm{H}^{+}$
Hence $\mathrm{H}_{2} \mathrm{SO}_{3}$ is the reducing agent because it undergoes oxidation.

Asked in: JEE-TOPICTESTS-CHEMISTRY

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