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# Need clarity, kindly explain! - Redox Reactions - NEET

For the redox reaction

$MnO_{4}^{-} + C_{2}O_{4}^{2-} + H^{+} \rightarrow Mn^{2+} + CO_{2} + H_{2}O$

the correct coefficients of the reactants for the balanced equation are

• Option 1)  $MnO_{4}^{-}$ $C_{2}O_{4}^{2-}$ $H^{+}$ 2 16 5

• Option 2)

 $MnO_{4}^{-}$ $C_{2}O_{4}^{2-}$ $H^{+}$ 2 5 16
• Option 3)

 $MnO_{4}^{-}$ $C_{2}O_{4}^{2-}$ $H^{+}$ 16 5 2
• Option 4)

 $MnO_{4}^{-}$ $C_{2}O_{4}^{2-}$ $H^{+}$ 5 16 2

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As we learnt

Balancing of Redox Reactions -

Oxidation number method

- wherein

1. Write the correct formula for each reactant and product.

2. Identify atom whose oxidation number is changed.

3. Calculate increase / decrease in oxidation number per atom and for the entire molecule / ion in which it occures.

4. Add $H^{+}/OH^{-}$ on appropriate side so that the total ionic charges of reactants and products are equal.

5. Make numbers of hydrogen atoms in the expression on the two sides equal by adding $H_{2}O$ to reactant or product

$2 MnO_{4}^{-} + 5 C_{2}O_{4}^{2-} + 16 H^{+}\rightarrow 2 Mn^{2+} + 10 CO_{2} + 8 H_{2}O$

Option 1)

 $MnO_{4}^{-}$ $C_{2}O_{4}^{2-}$ $H^{+}$ 2 16 5

This is incorrect.

Option 2)

 $MnO_{4}^{-}$ $C_{2}O_{4}^{2-}$ $H^{+}$ 2 5 16

This is correct.

Option 3)

 $MnO_{4}^{-}$ $C_{2}O_{4}^{2-}$ $H^{+}$ 16 5 2

This is incorrect.

Option 4)

 $MnO_{4}^{-}$ $C_{2}O_{4}^{2-}$ $H^{+}$ 5 16 2

This is incorrect.

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