Question

3ag{s} + Au{No3}3{aq} > Au{s} +3AgNO3{s)

Write a balanced net ionic equation for the reaction.
Identify which reactant is oxidized and which one is reduced.
Identify which reactant is the oxidizing agent and which one is the reducing agent.
Write balanced half reactions for the oxidation and reduction.

Answer 1

For the given reaction

$3Ag_{(s)}+Au(NO_3)_{3(aq)} \rightarrow Au_{(s)}+3AgNO_{3(aq)}$

a balanced net ionic equation is

$3Ag_{(s)}+Au^{3+}_{(aq)} \rightarrow Au_{(s)}+3Ag^+_{(aq)}$

During the reaction

Ag_(s) is oxidized and it is the reducing agent,

Au(NO₃)_3(aq) is reduced and it is the oxidizing agent.

The balanced half reactions for the oxidation and reduction are following:

$3Ag_{(s)} \rightarrow 3Ag^+_{(aq)} + 3e^-$ (oxidation half-reaction)

$Au^{3+}_{(aq)}+3e^- \rightarrow Au_{(s)}$ ​ (reduction half-reaction)