Question

Zn sub (s) + FeCl sub 2(aq), reaction arrow, Fe sub (s) + ZnCl sub 2(aq)

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

$Zn_{(s)}+FeCl_{2(aq)} \rightarrow Fe_{(s)}+ZnCl_{2(aq)}$

a balanced net ionic equation is

$Zn_{(s)}+Fe^{2+}_{(aq)} \rightarrow Fe_{(s)}+Zn^{2+}_{(aq)}$

During the reaction

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

FeCl_2(aq) is reduced and it is the oxidizing agent.

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

$Zn_{(s)} \rightarrow Zn^{2+}_{(aq)} + 2e^-$ (oxidation half-reaction)

$Fe^{2+}_{(aq)}+2e^- \rightarrow Fe_{(s)}$ (reduction half-reaction)