Question

A solution contains Fe²⁺, Fe³⁺ and I⁻ ions. This solution
was treated with iodine at 35°C. E° for Fe³⁺ / Fe²⁺ is + 0.77 V
and E° for I₂/2I⁻ = 0.536 V. The favourable redox reaction is :
(a) I₂ will be reduced to I⁻
(b) There will be no redox reaction
(c) I⁻ will be oxidised to I₂
(d) Fe²⁺ will be oxidised to Fe³⁺

Answer 1

Explanation:

Answer: The favorable redox reaction is written below.

Explanation:

For the reaction to be spontaneous, the Gibbs free energy of the reaction must come out to be negative.

Relationship between standard Gibbs free energy and standard electrode potential follows:

For a reaction to be spontaneous, the standard electrode potential must be positive.

To calculate the of the reaction, we use the equation:

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

We are given:

Calculating the using above equation, we get:

Here, iron will get reduced and iodine will get oxidized.

Half reaction follows:

Oxidation half reaction:  

Reduction half reaction:      ( ×  2)

Net redox reaction follows:

Hence, the favorable redox reaction is written above

Answer 2

Explanation:

A solution contains Fe²⁺, Fe³⁺ and I⁻ ions. This solution

was treated with iodine at 35°C. E° for Fe³⁺ / Fe²⁺ is + 0.77 V

and E° for I₂/2I⁻ = 0.536 V. The favourable redox reaction is :

(a) I₂ will be reduced to I⁻

(b) There will be no redox reaction✔️

(c) I⁻ will be oxidised to I₂

(d) Fe²⁺ will be oxidised to Fe³⁺