Balance the following equation by oxidation number method-
Fe2+ + Cr2O72- + H+ ---- Fe3+ + Cr3- + H2O
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Solution
Equation-
Fe2+ + Cr2O72- + H+ Fe3+ + Cr3+ + H2O
The oxidation number of chromium decreases from +6 in Cr2O72 to +3 in Cr3+. The total decrease for two chromium atoms in Cr2O72- to Cr3+ is 6. On the other hand, the oxidation number of iron increases from +2 (in Fe2+) to +3 (in Fe3+).
To balance increase and decrease of oxidation numbers, multiply Fe2+ by 6 and Cr2O72- by 1. Then we get,
6Fe2+ + Cr2O72- + H+ Fe3+ + Cr3+ + H2O
Balancing Fe and Cr atoms on both side of reaction.
6Fe2+ + Cr2O72- + H+ 6Fe3+ + 2Cr3+ + H2O
To balance O atoms multiply H2O by 7
6Fe2+ + Cr2O72- + H+ 6Fe3+ + 2Cr3+ + 7H2O
To balance H-atoms multiply H+ by 14
6Fe2+ + Cr2O72- + 14H+ 6Fe3+ + 2Cr3+ + 7H2O