Answer to Question #252048 in Chemistry for sert

Question

Identify the reactant oxidized and the reactant reduced in the following equations;

1. Cl₂(g) + 2 K(s) → 2 KCl(s)
2. FeSO4(aq) + Mg(s) → Fe(s) + MgSO4(aq)
3. Ni_(s) + Pb²⁺_(aq) →Pb_(s) + Ni²⁺_(aq)

Answer 1

An atom is oxidized if its oxidation number increases, the reducing agent, and an atom is reduced if its oxidation number decreases, the oxidizing agent.

1.Cl₂(g) + 2 K(s) → 2 KCl(s)

Chlorine initially has oxidation number 0; after reaction, its oxidation number is -1. Its oxidation number increases, so that Chlorine is reduced.

Potassium initially has oxidation number 0; after reaction, its oxidation number is +1. Its oxidation number decreases, so that Potassium is oxidized.

2.FeSO4(aq) + Mg(s) → Fe(s) + MgSO4(aq)

Iron initially has oxidation number +2; after reaction, its oxidation number is 0. Its oxidation number decreases, so that Iron is oxidized.

Magnesium initially has oxidation number 0; after reaction, its oxidation number is +2. Its oxidation number increases, so that Magnesium is reduced.

3.Ni_(s) + Pb²⁺_(aq) →Pb_(s) + Ni²⁺_(aq)

Nickel initially has oxidation number 0; after reaction, its oxidation number is +2. Its oxidation number increases, so that Nickel is reduced.

Lead initially has oxidation number +2; after reaction, its oxidation number is 0. Its oxidation number decreases, so that Lead is oxidized.