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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.

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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.

The study of chemicals and bonds is called chemistry. The reaction which has both oxidation and reduction is called a redox reaction.

The correct answer to the question is mentioned below.

What is the balanced reaction?

  • Balancing reactions ensure that all atoms present in the starting materials are accounted for in the final compounds.

The balanced reaction of the given question is as follows:-

[tex]Part A : Zn(s) + Sn^{2+}(aq) ---> Zn^{2+}(aq) + Sn(s).\\ Part B : 3Mg(s) + 2Cr^{3+}(aq) ----> 3Mg^{2+}(aq) + 2Cr(s).\\ Part C: 3MnO^-_2 + 24H^+ 5Al------> 5Al^3+ + 3Mn^{2+} + 12H_2O. [/tex]

Hence, the correct answer to the question is mentioned below.

For more information about the balanced reaction, refer to the link:-

https://brainly.com/question/1291604

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