Write the anodic reaction for the electrolysis of concentrated zinc chloride solution.

(a) Using plantium electrodes.
(b) Using zinc electrodes

a. At the anode you have 2Cl^- ==> Cl2 + 2e.

b. What do you think the Cl2 will react with?

Zn + e

Zinc

(a) To determine the anodic reaction for the electrolysis of concentrated zinc chloride solution using platinum electrodes, you need to consider the reduction potentials of the species involved.

1. Write down the balanced equation for the dissociation of zinc chloride:
ZnCl2 ⇌ Zn²⁺ + 2Cl⁻

2. Next, identify the reduction potentials of the species involved. The species with the more positive reduction potential will be reduced (cathodic reaction), while the other species will be oxidized (anodic reaction).

The possible reactions involving platinum electrodes are:
Zn²⁺ + 2e⁻ → Zn (at cathode, reduction)
2Cl⁻ → Cl₂ + 2e⁻ (at anode, oxidation)

Therefore, the anodic reaction using platinum electrodes for the electrolysis of concentrated zinc chloride solution is:
2Cl⁻ → Cl₂ + 2e⁻

(b) Now, let's determine the anodic reaction for the electrolysis of concentrated zinc chloride solution using zinc electrodes.

The presence of zinc electrodes means that zinc will take part in the anodic reaction.

1. Write down the balanced equation for the dissociation of zinc chloride:
ZnCl2 ⇌ Zn²⁺ + 2Cl⁻

2. Identify the possible anodic reactions involving zinc:
Zn → Zn²⁺ + 2e⁻ (oxidation of zinc)
2Cl⁻ → Cl₂ + 2e⁻ (oxidation of chloride ions)

Since we want to determine the anodic reaction involving zinc, we will use the oxidation of zinc:

Zn → Zn²⁺ + 2e⁻

Therefore, the anodic reaction using zinc electrodes for the electrolysis of concentrated zinc chloride solution is:
Zn → Zn²⁺ + 2e⁻