Question

[30 Points]

Consider the incomplete reaction (partial ionic equation) given below:

A) Cu^2+ + Zn --> Zn^2+ + Cu

I) Give the two half equations for this reaction; oxidation + reduction

II) Identify the chemical substance (species) that has undergone oxidation

III) Identify the chemical substance (species) that has undergone reduction

IV) Identify (from the reactants) the oxidizing agent (oxidant) in this reaction:

V) Identify (from the reactants) the reducing agent (reductant) in this reaction: ​

Answer 1

Step-by-step explanation:

• For 1:

Oxidation reaction is defined as the reaction when a substance looses its electrons.

`X\rightarrow X^(n+)+ne^-`

Reduction reactions are defined as the reactions when a substance gains electrons.

`X^(n+)+ne^-\rightarrow X`

For the given reaction:

`Cu^(2+)+Zn\rightarrow Zn^(2+)+Cu`

Oxidation half-cell reaction:
`Zn\rightarrow Zn^(2+)+2e^-`

Reduction half-cell reaction:
`Cu^(2+)+2e^-\rightarrow Cu`

• For 2 & 3:

The species which looses electrons is undergoing an oxidation reaction and the species which gains electrons is undergoing a reduction reaction.

Here, species undergoing oxidation is Zinc and species undergoing reduction is copper.

• For 4:

Oxidizing agents are the species which oxidizes the other species and itself gets reduced.

Here, the oxidizing agent is Copper.

• For 5:

Reducing agents are the species which reduces the other species and itself gets oxidized.

Here, the reducing agent is Zinc.