Consider the reaction H_2SO_{3(aq)} + Sn^{4+} | vedclass

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Question

(C) In the given reaction: $\overset{+4}{H_2SO_3}_{(aq)} + Sn^{4+}_{(aq)} + H_2O_{(l)} 	o Sn^{2+}_{(aq)} + \overset{+6}{HSO_4^-}_{(aq)} + 3H^{+}_{(aq

Vedclass · Accepted Answer

$H_2SO_3$ is the reducing agent because it undergoes oxidation

Vedclass · Answer

(C) In the given reaction: $\overset{+4}{H_2SO_3}_{(aq)} + Sn^{4+}_{(aq)} + H_2O_{(l)} 	o Sn^{2+}_{(aq)} + \overset{+6}{HSO_4^-}_{(aq)} + 3H^{+}_{(aq)}$.$1$. The oxidation state of $S$ in $H_2SO_3$ increases from $+4$ to $+6$,which means $H_2SO_3$ undergoes oxidation.$2$. The oxidation state of $Sn$ decreases from $+4$ to $+2$,which means $Sn^{4+}$ undergoes reduction.$3$. Since $H_2SO_3$ undergoes oxidation,it acts as the reducing agent.Therefore,the correct statement is that $H_2SO_3$ is the reducing agent because it undergoes oxidation.

Consider the reaction $H_2SO_{3(aq)} + Sn^{4+}_{(aq)} + H_2O_{(l)} \to Sn^{2+}_{(aq)} + HSO_4^-(aq) + 3H^{+}_{(aq)}$. Which of the following statements is correct?

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