Answer to Question #92643 in Organic Chemistry for Lee

Question

zn(s) + pb(no3)2(aq) Pb{s} + Zn{NO3) 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

​$Zn_{(s)}+Pb(NO_3)_{2(aq)} \rightarrow Pb_{(s)}+Zn(NO_3)_{2(aq)}$

a balanced net ionic equation is

​$Zn_{(s)}+Pb^{2+}_{(aq)} \rightarrow Pb_{(s)}+Zn^{2+}_{(aq)}$

During the reaction

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

Pb(NO₃)_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)

$Pb^{2+}_{(aq)} +2e^- \rightarrow Pb_{(s)}$ ​ (reduction half-reaction)