Zn → Zn2+ + 2e−

8e− + 10H+ + NO3− → NH4+ + 3H2O
4Zn + 10H+ + NO3− → 4Zn2+ + NH4+ + 3H2O
Operate eq. (1) × 4 + eq. (2) × 1
Zn + Zn2+ + 2e−

Correct answer: 4Zn + 10H+ + NO3− → 4Zn2+ + NH4+ + 3H2O

Solution

Option B represents the balanced redox reaction where zinc is oxidized to Zn2+ and nitrate is reduced to ammonium ion, maintaining charge and mass balance.

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