Question

Consider the redox reaction below.

Mg(s) + Fe2+ (aq) —>Mg2+ (aq) + Fe(s)
Which equation is a half reaction that describes the reduction that is taking place?
Fe2+ (aq) + 22 -> Fe(s)
Mg(s) — Mg2+ (aq) + 2e
Fe2+ (aq) –>Fe(s) + 2e-
Mg(s)+2e--> Mg2+ (aq)

Answer 1

Fe2+ (aq) + 2e -> Fe(s)

Step-by-step explanation:

Oxidation:

Oxidation involve the removal of electrons and oxidation state of atom of an element is increased.

Reduction:

Reduction involve the gain of electron and oxidation number is decreased.

Consider the following reaction:

Mg(s) + Fe2+ (aq) —>Mg2+ (aq) + Fe(s)

Magnesium loses its two valance electrons and oxidized while iron accept two electrons get reduced.

Magnesium is reducing agent while iron is oxidizing agent.

Oxidizing agents:

Oxidizing agents oxidize the other elements and itself gets reduced.

Reducing agents:

Reducing agents reduced the other element are it self gets oxidized.