(A) The balanced chemical reaction is:$2 MnO_{4}^{-} + 5 SO_{3}^{2-} + 6 H^{+} \rightarrow 2 Mn^{2+} + 5 SO_{4}^{2-} + 3 H_{2}O$From the balanced chem

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(A) The balanced chemical reaction is:$2 MnO_{4}^{-} + 5 SO_{3}^{2-} + 6 H^{+} \rightarrow 2 Mn^{2+} + 5 SO_{4}^{2-} + 3 H_{2}O$From the balanced chemical equation,we can observe that:$5$ moles of $SO_{3}^{2-}$ react with $2$ moles of $KMnO_4$.Therefore,$1$ mole of $SO_{3}^{2-}$ reacts with $2/5$ moles of $KMnO_4$.Hence,the correct option is $A$.

Class 11 Chemistry Redox Reactions Redox reaction and Method for balancing Redox reaction

Medium

The number of moles of acidified $KMnO_4$ required to convert one mole of sulphite ion into sulphate ion is

A
$2/5$
B
$3/5$
C
$4/5$
D
$1$

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Class 11

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Redox Reactions

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Redox reaction and Method for balancing Redox reaction

What is the value of $x$ and $y$ in order to balance the following redox reaction?
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When copper is heated with concentrated $HNO_3$,it produces:

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How many moles of $K_2Cr_2O_7$ can be reduced by $1 \ mol$ of $Sn^{2+}$?

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Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$Na_2CrO_4 + HCl \longrightarrow H_2Cr_2O_7 + NaCl$

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In the balanced chemical reaction $IO_3^- + aI^- + bH^+ \longrightarrow cH_2O + dI_2$,the values of $a, b, c,$ and $d$ are respectively:

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The number of moles of acidified $KMnO_4$ required to convert one mole of sulphite ion into sulphate ion is

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What is the value of $x$ and $y$ in order to balance the following redox reaction?$x CuO + y NH_3 \longrightarrow x Cu + N_2 + x H_2 O$

When copper is heated with concentrated $HNO_3$,it produces:

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What is the value of $x$ and $y$ in order to balance the following redox reaction?
$x CuO + y NH_3 \longrightarrow x Cu + N_2 + x H_2 O$

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$Na_2CrO_4 + HCl \longrightarrow H_2Cr_2O_7 + NaCl$