Question

Exercise 18.44

Label the anode and cathode, indicate the direction of electron flow and the species present in each solution for each of the following overall redox reactions.

Part A

Ni2+(aq)+Mg(s)→Ni(s)+Mg2+(aq)

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Part B

Indicate the half-reaction occurring at Anode.

Express your answer as a chemical equation. Identify all of the phases in your answer.

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Part C

Indicate the half-reaction occurring at Cathode.

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Part D

2H+(aq)+Fe(s)→H2(g)+Fe2+(aq)

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Part E

Indicate the half-reaction occurring at Anode.

Express your answer as a chemical equation. Identify all of the phases in your answer.

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Part F

Indicate the half-reaction occurring at Cathode.

Express your answer as a chemical equation. Identify all of the phases in your answer.

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Part G

2NO−3(aq)+8H+(aq)+3Cu(s)→2NO(g)+4H2O(l)+3Cu2+(aq)

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Part H

Indicate the half-reaction occurring at Anode.

Express your answer as a chemical equation. Identify all of the phases in your answer.

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Part I

Indicate the half-reaction occurring at Cathode.

Express your answer as a chemical equation. Identify all of the phases in your answer.

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Answer 1

A) Ni2+(aq) + Mg(s) --> Mg2+(aq) + Ni(s)

--> Half cell reaction at cathode (reduction);

Ni2+(aq) + 2e- ---> Ni(s)

---> Half cell reaction at anode (oxidation)

Mg(s) --> Mg2+(aq) + 2e-

--> Electron will flow from anode to cathode i.e. Mg2+ to Ni2+.

--> Ions will be Ni2+ in cathode solution and Mg2+ in anode solution

D) 2H+(aq) + Fe(s) --> Fe2+(aq) + H2(g)

--> Half cell reaction at cathode (reduction);

2H+(aq) + 2e- --> H2(g)

--> At anode (oxidation);

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

---> ions present in cathode H+ and in anode Fe2+

--> Electron will from Fe2+ to H+

G)

---> half cell reaction at cathode (reduction);

2NO3 -(aq) + 8H+(aq) + 6e- --> 2NO(g) + 4H2O(l)

---> Anodic reaction (oxidation);

3Cu(s) ---> 3Cu2+(aq) + 6e-

--> Electron will flow from Cu2+ to NO3 -

--> Anodic ion species = Cu2+

Cathodic ion species = NO3 - , H+

Let me know if any doubt.