Answer to Question #170867 in Organic Chemistry for Jeremy

Question

• 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.

a. FeCl2 + Zn = ZnCl2 + Fe

b. Zn + pb(NO3)2 = pb + Zn(NO3)2

c. 3Ag + Au(NO3)3 = Au + 3AgNO3

d. 3Mg + Al2(SO4)3 = 2Al + 3MgSO4

Answer 1

a) The balanced net ionic equation ;

During the reaction;

Zn(s) is oxidized and it is the reducing agent,FeCl2(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-equation)

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

b) The balanced net ionic equation ;

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) 

c) The balanced net ionic equation ;

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)

d) The balanced net ionic equation ;

During the reaction;

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

Al₂(SO₄)_3(aq) is reduced and it is the oxidizing agent.The balanced half reactions for the oxidation and reduction are following:

$3Mg_{(s)} \rightarrow 3Mg^{2+}_{(aq)}+6e^-$ (oxidation half reaction)

$2Al^{3+}_{(aq)}+6e^- \rightarrow 2Al_{(s)}$ (reduction half reaction)