Question

Use the half-reaction method to balance each redox reaction occurring in acidic aqueous solution. Pb(s)+NO3−(aq)⟶Pb2+(aq)+NO(g) Express your answer as a chemical equation. Identify all of the phases in your answer.

Answer 1

To balance the redox reaction Pb(s) + NO3-(aq) → Pb2+(aq) + NO(g) using the half-reaction method, the balanced equation in acidic solution is 3Pb(s) + 2NO3-(aq) + 8H+(aq) → 3Pb2+(aq) + 2NO(g) + 4H2O(l).

Step-by-step explanation:

The question asks to use the half-reaction method to balance the redox reaction between lead (Pb) and nitrate ions (NO3-) in an acidic solution, resulting in Pb2+ and nitrogen monoxide (NO).

To do this, we will separate the reaction into two half-reactions - one for oxidation and one for reduction - and then balance each one before combining them for the overall balanced equation.

Oxidation Half-Reaction:

Pb(s) → Pb2+(aq) + 2e-

Reduction Half-Reaction:

NO3-(aq) + 4H+(aq) + 3e- → NO(g) + 2H2O(l)

Combined Balanced Reaction:

3Pb(s) + 2NO3-(aq) + 8H+(aq) → 3Pb2+(aq) + 2NO(g) + 4H2O(l)