Balance each of the following redox reactions occurring in acidic aqueous solution.

Part A

Zn (s) + Sn2 + (aq) →Zn2 + (aq) + Sn (s) Express your answer as a chemical equation. Identify all of the phases in your answer.

Part B

Mg (s) + Cr3 + (aq) →Mg2 + (aq) + Cr (s) Express your answer as a chemical equation. Identify all of the phases in your answer.

Part C

MnO4 - (aq) + Al (s) →Mn2 + (aq) + Al3 + (aq) Express your answer as a chemical equation. Identify all of the phases in your answer.

Part A : Zn (s) + Sn²⁺ (aq) → Zn²⁺ (aq) + Sn (s).

Part B : 3Mg (s) + 2Cr³⁺ (aq) → 3Mg²⁺ (aq) + 2Cr (s).

Part C: 3MnO₄⁻ + 24H⁺ + 5Al → 5Al³⁺ + 3Mn²⁺ + 12H₂O.

Explanation:

Part A : Zn (s) + Sn²⁺ (aq) → Zn²⁺ (aq) + Sn (s), Express your answer as a chemical equation. Identify all of the phases in your answer.

It is balanced as written: Zn (s) + Sn²⁺ (aq) → Zn²⁺ (aq) + Sn (s).

The two half reactions are:

The oxidation reaction: Zn (s) → Zn²⁺ (aq) + 2e.

The reduction reaction: Sn²⁺ (aq) + 2e → Sn (s).

To obtain the net redox reaction, we add the two-half reactions as the no. of electrons in the two-half reactions is equal.

So, the net chemical equation is:

Zn (s) + Sn²⁺ (aq) → Zn²⁺ (aq) + Sn (s).

Part B: Mg (s) + Cr³⁺ (aq) → Mg²⁺ (aq) + Cr (s), Express your answer as a chemical equation. Identify all of the phases in your answer.

To balance and write the net chemical equation, we should write the two-half reactions:

The two half reactions are:

The oxidation reaction: Mg (s) → Mg²⁺ (aq) + 2e.

The reduction reaction: Cr³⁺ (aq) + 3e → Cr (s).

To obtain the net redox reaction, we multiply the oxidation reaction by 3 (3Mg (s) → 3Mg²⁺ (aq) + 6e) and the reduction reaction by 2 (2Cr³⁺ (aq) + 6e → 2Cr (s)) to equalize the no. of electrons in the two-half reactions.

So, the net redox reaction will be:

3Mg (s) + 2Cr³⁺ (aq) → 3Mg²⁺ (aq) + 2Cr (s).

Part C : MnO⁴⁻ (aq) + Al (s) → Mn²⁺ (aq) + Al³⁺ (aq), Express your answer as a chemical equation. Identify all of the phases in your answer.

To balance and write the net chemical equation, we should write the two-half reactions:

The two half reactions are:

The oxidation reaction: Al → Al³⁺ + 3e.

The reduction reaction: MnO₄⁻ + 8H⁺ + 5e → Mn²⁺ + 4H₂O.

To obtain the net redox reaction, we multiply the oxidation reaction by 5 (5Al → 5Al³⁺ + 15e) and the reduction reaction by 3 (3MnO₄⁻ + 24H⁺ + 15e → 3Mn²⁺ + 12H₂O) to equalize the no. of electrons in the two-half reactions.

So, the net redox reaction will be:

3MnO₄⁻ + 24H⁺ + 5Al → 5Al³⁺ + 3Mn²⁺ + 12H₂O.