Consider the following redox reaction: Ag⁺(aq) + Fe²⁺(aq) ⇌ Ag(s) + Fe³⁺(aq). How many moles of electrons are exchanged?

In the redox reaction Ag⁺(aq) + Fe²⁺(aq) ⇌ Ag(s) + Fe³⁺(aq),

1 mole of electrons is exchanged.

Let's consider the following balanced redox reaction.

Ag⁺(aq) + Fe²⁺(aq) ⇌ Ag(s) + Fe³⁺(aq).

We can identify both half-reactions.

We can conclude that:

In the redox reaction Ag⁺(aq) + Fe²⁺(aq) ⇌ Ag(s) + Fe³⁺(aq),

1 mole of electrons is exchanged.

Learn more: link

1 mol of electron is exchanged. The mol of electrons that is released by the iron, is gained by the silver.

Explanation:

We need to determine the half reactions:

Ag⁺ → Ag

These is the reduction reaction, where Silver decreases the oxidation state. It gained 1 mol of e⁻

Fe²⁺ → Fe³⁺

In this case, iron increases the oxidation state, from +2 to +3. It has released 1 mol of electrons. This is the oxidation reaction.

The complete redox is:

Ag⁺ + 1e⁻ → Ag

Fe²⁺ → Fe³⁺ + 1e⁻

Ag⁺(aq) + 1e⁻ + Fe²⁺(aq) ⇌ Ag(s) + Fe³⁺(aq) + 1e⁻

The electrons will be cancelled.

< > according to newton's third law of motion, forces always act in equal but opposite pairs. another way of saying this is for every action, there is an equal but opposite reaction.< >