Answer to Question #92646 in Organic Chemistry for Lee

Question

3mg s al2(so4)3 > 2Al{s} +3MgSO4

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

$3Mg_{(s)}+Al_2(SO_4)_{3(aq)} \rightarrow 2Al_{(s)}+3MgSO_{4(aq)}$

​a balanced net ionic equation is

​$3Mg_{(s)}+2Al^{3+}_{(aq)} \rightarrow 2Al_{(s)}+3Mg^{2+}_{(aq)}$

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)