Problem: Balance the following redox reaction by inserting the appropriate coefficients.H+ + CrO42- + NO2- → Cr3+ + H2O +NO3-

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We’re being asked to balance the given oxidation-reduction reaction:

H+ + CrO42– + NO2 Cr3+ + H2O + NO3


We assume that the redox is in acidic solution since H+ is present. When balancing redox reactions under acidic conditions, we will follow the following steps.

Step 1: Separate the whole reaction into two half-reactions.

Step 2: Balance the non-hydrogen and non-oxygen elements first.

Step 3: Balance oxygen by adding H2O to the side that needs oxygen. (1 O: 1 H2O)

Step 4: Balance hydrogen by adding H+ to the side that needs hydrogen. (1 H: 1 H+)


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Problem Details

Balance the following redox reaction by inserting the appropriate coefficients.

H+ + CrO42- + NO2- → Cr3+ + H2O +NO3-