Question

Consider the reaction below.

2 upper I superscript minus (a q) plus upper C l subscript 2 (g) right arrow 2 upper C l minus (a q) plus upper I subscript 2 (a q).

Which half reaction correctly describes the reduction that is taking place?
Upper C l subscript 2 9 g) plus e superscript minus right arrow 2 upper C l superscript minu (a).
Upper C l subscript 2 (g) plus e superscript minus right arrow 2 upper C l superscript minus (a q).
2 upper I superscript minus (a q) right arrow upper I subscript 2 (a q) plus 2 e subscript minus.
2 upper I superscript minus (a q) right arrow upper I subscript 2 (a q) plus e superscript minus.

Answer 1

A

Step-by-step explanation:

It's A

Answer 2

2 e⁻ + Cl₂(g) → 2 Cl⁻(aq)

Step-by-step explanation:

Let's consider the following balanced redox equation.

2 I⁻(aq) + Cl₂(g) → 2 Cl⁻(aq) + I₂(aq)

We can identify 2 half-reactions:

Oxidation: 2 I⁻(aq) → I₂(aq) + 2 e⁻

Reduction: 2 e⁻ + Cl₂(g) → 2 Cl⁻(aq)

We can identify the second half-reaction as the reduction reaction because Cl₂ gains 2 electrons and its oxidation number decreases from 0 to 1-.