How many moles of H_2SO_3 are required to red | vedclass

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(C) In an acidic medium,the redox reaction between $KMnO_4$ and $H_2SO_3$ is given by the balanced equation:$2KMnO_4 + 5H_2SO_3 \longrightarrow K_2SO_

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$2.5$

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(C) In an acidic medium,the redox reaction between $KMnO_4$ and $H_2SO_3$ is given by the balanced equation:$2KMnO_4 + 5H_2SO_3 \longrightarrow K_2SO_4 + 2MnSO_4 + 2H_2SO_4 + H_2O$From the stoichiometry of the balanced equation,$2 	ext{ moles}$ of $KMnO_4$ react with $5 	ext{ moles}$ of $H_2SO_3$.Therefore,$1 	ext{ mole}$ of $KMnO_4$ requires $\frac{5}{2} = 2.5 	ext{ moles}$ of $H_2SO_3$.

How many moles of $H_2SO_3$ are required to reduce one mole of $KMnO_4$ in an acidic medium?

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