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Fe2S3 + HNO3 ? Fe(NO3)3 + NO2 + S 1) Balance this redox reaction in Acidic...

Fe2S3 + HNO3 ? Fe(NO3)3 + NO2 + S

1) Balance this redox reaction in Acidic conditions.

2) Identify the oxidizing and reducing agent

3) List the number of electrons transferred in the reaction (n).

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Answer #1

1) First balance all atoms except H and O.

The oxidation number of S changes from -2 to 0. The net increase in the oxidation number for 3 S atoms is 6.

The oxidation number of N changes from +5 (in nitric acid) to +4 (in nitrogen dioxide)

The net decrease in the oxidation number is 1.

To balance the net increase in the oxidation number with net decrease in the oxidation number, multiply nitric acid with 12 and nitrogen dioxide with 6.

Balance O atoms by adding six water molecules on RHS. H atoms are balanced.

The above equation is balanced.

2) Nitric acid is the oxidizing agent and is the reducing agent.

3) Six electrons are transferred in the reaction.

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