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Question

Balance the following reaction.

Cr2O27+C2H4O+H+C2H4O2+Cr3+

A
Cr2O27+3C2H4O+8H+3C2H4O2+2Cr3++4H2O
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B
Cr2O27+C2H4O+8H+3C2H4O2+5Cr3++H2O
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C
Cr2O27+4C2H4O+4H+C2H4O2+2Cr3++4H2O
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D
None of these
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Solution

The correct option is C Cr2O27+3C2H4O+8H+3C2H4O2+2Cr3++4H2O
The unbalanced redox equation is as follows:
Cr2O27+C2H4O+H+C2H4O2+Cr3+
Balance all atoms other than H and O.
Cr2O27+C2H4O+H+C2H4O2+2Cr3+
The oxidation number of Cr changes from 6 to 3. So the change in oxidation number of one Cr atom is 3.
For 2 Cr atoms, the oxidation number changes by 6.
The oxidation number of C changes from -1 to 0. So the change in oxidation number of 1 C atom is 1.
For 2 C atoms, the oxidation number changes by 2.
The increase in the oxidation number is balanced with decrease in the oxidation number by multiplying
C2H4O and C2H4O2 with 3.
Cr2O27+3C2H4O+H+3C2H4O2+2Cr3+

O atoms are balanced by adding 4 water molecules on RHS.
Cr2O27+3C2H4O+H+3C2H4O2+2Cr3++4H2O
Hydrogen atoms are balanced by adding 7 H+ atoms on RHS.
Cr2O27+3C2H4O+8H+3C2H4O2+2Cr3++4H2O
This is the balanced chemical equation.

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