Write balanced chemical equation for the following reactions: Permanganate ion \[\ce{(MnO^{-}4)}\] reacts with sulphur dioxide gas in acidic medium to produce \[\ce{Mn^{2+}}\] and hydrogen sulphate ion.

\[\ce{2MnO^{-}4 + 5SO2 + 2H2O + H+ -> 5HSO^{-}4 + 2Mn^{2+}}\] Balancing by ion-electron method: \[\ce{\overset{+7}{Mn}\overset{-2}{O}^{-}4 + \overset{+4}{S}\overset{-2}{O2} -> \overset{+2}{Mn}^{2+} + \overset{+1}{H}\overset{+6}{S}\overset{-2}{O}^{-}4}\] (Skeletal equation) Oxidation half: \[\ce{SO2 -> HSO^{-}4}\] Reduction half: \[\ce{MnO^{-}4 -> Mn^{2+}}\] Oxidation half: \[\ce{SO2 -> HSO^{-}4 + 2e-}\] \[\ce{SO2 + 2H2O -> HSO^{-}4 + 3H^{+} + 2e-}\] ......(i) (Add \[\ce{2H2O}\] molecules to balance \[\ce{O}\] atoms) Reduction half: \[\ce{MnO^{-}4 + 5e- -> Mn^{2+}}\] \[\ce{MnO^{-}4 + 8H^{+} + 5e- -> Mn^{2+} + 4H2O}\] ......(ii) (Add \[\ce{4H2O}\] molecules to balance \[\ce{O}\] atoms and \[\ce{H}\] atoms) Add oxidation and reduction half \[\ce{[SO2 + 2H2O -> HSO^{-}4 + 3H+ + 2e-] × 5}\] \[\ce{[MNO^{-}4 + 8H+ + 5e- -> Mn^{2+} + 4H2O] × 2}\] \[\ce{2MNo^{-}4 + 5SO2 + 2H2O + H+ -> 5HSO^{-}4 + 2Mn^{2+}}\]

Write balanced chemical equation for the following reactions: Permanganate ion (MnOX4−) reacts with sulphur dioxide gas in acidic medium to produce MnX2+ and hydrogensulphate ion. - Chemistry

प्रश्न

Write balanced chemical equation for the following reactions:

Permanganate ion $(MnO_{4}^{-})$ reacts with sulphur dioxide gas in acidic medium to produce $Mn^{2 +}$ and hydrogen sulphate ion.

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उत्तर

$2 MnO_{4}^{-} + 5 SO_{2} + 2 H_{2} O + H^{+} ⟶ 5 HSO_{4}^{-} + 2 Mn^{2 +}$

Balancing by ion-electron method:

$\overset{+ 7}{Mn} \overset{- 2}{O}_{4}^{-} + \overset{+ 4}{S} \overset{- 2}{O_{2}} ⟶ \overset{+ 2}{Mn}^{2 +} + \overset{+ 1}{H} \overset{+ 6}{S} \overset{- 2}{O}_{4}^{-}$ (Skeletal equation)

Oxidation half: $SO_{2} ⟶ HSO_{4}^{-}$

Reduction half: $MnO_{4}^{-} ⟶ Mn^{2 +}$

Oxidation half: $SO_{2} ⟶ HSO_{4}^{-} + 2 e^{-}$

$SO_{2} + 2 H_{2} O ⟶ HSO_{4}^{-} + 3 H^{+} + 2 e^{-}$ ......(i)

(Add $2 H_{2} O$ molecules to balance $O$ atoms)

Reduction half:

$MnO_{4}^{-} + 5 e^{-} ⟶ Mn^{2 +}$

$MnO_{4}^{-} + 8 H^{+} + 5 e^{-} ⟶ Mn^{2 +} + 4 H_{2} O$ ......(ii)

(Add $4 H_{2} O$ molecules to balance $O$ atoms and $H$ atoms)

Add oxidation and reduction half

$[SO_{2} + 2 H_{2} O ⟶ HSO_{4}^{-} + 3 H^{+} + 2 e^{-}] \times 5$

$[MNO_{4}^{-} + 8 H^{+} + 5 e^{-} ⟶ Mn^{2 +} + 4 H_{2} O] \times 2$

$2 MNo_{4}^{-} + 5 SO_{2} + 2 H_{2} O + H^{+} ⟶ 5 HSO_{4}^{-} + 2 Mn^{2 +}$

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Balancing Redox Reactions in Terms of Loss and Gain of Electrons

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Q 21.(i)Q 20 Q 21.(ii)

अध्याय 8: Redox Reactions - Multiple Choice Questions (Type - I) [पृष्ठ १०८]

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एनसीईआरटी एक्झांप्लर Chemistry [English] Class 11

अध्याय 8 Redox Reactions
Multiple Choice Questions (Type - I) | Q 21.(i) | पृष्ठ १०८

Write balanced chemical equation for the following reactions: Permanganate ion (MnOX4−) reacts with sulphur dioxide gas in acidic medium to produce MnX2+ and hydrogensulphate ion. - Chemistry

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Write balanced chemical equation for the following reactions: Permanganate ion (MnOX4−) reacts with sulphur dioxide gas in acidic medium to produce MnX2+ and hydrogensulphate ion. - Chemistry

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