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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
 
Answers (1)
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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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