Question

Identify both the oxidizing agent and the reducing agent in the following oxidation-reduction reaction. Fe(s) + 2 Ag⁺(aq) → Fe²⁺(aq) + 2 Ag(s)

o Fe²⁺ (aq) is the reducing agent and Ag (aq) is the oxidizing agent.
o Ag(s) is the reducing agent and Fe(s) is the oxidizing agent.
o Ag⁺ (aq) is the reducing agent and Fe²⁺(aq) is the oxidizing agent.
O Ag⁺ (aq) is the reducing agent and Fe(s) is the oxidizing agent.
o Fe(s) is the reducing agent and Ag⁺ (aq) is the oxidizing agent.

Answer 1

In the redox reaction Fe(s) + 2 Ag⁺(aq) → Fe²⁺(aq) + 2 Ag(s), iron (Fe) is oxidized and acts as the reducing agent whereas silver ions (Ag⁺(aq)) are reduced and act as the oxidizing agent.

Step-by-step explanation:

To identify the oxidizing agent and reducing agent in the given redox reaction, Fe(s) + 2 Ag⁺(aq) → Fe²⁺(aq) + 2 Ag(s), we need to determine which species are oxidized and which are reduced.

The iron (Fe) starts as a solid metal (Fe(s)) and is oxidized to Fe²⁺(aq), losing two electrons in the process. The oxidation of iron means it is the reducing agent since it donates electrons.

On the other hand, silver ions (Ag⁺(aq)) gain electrons and are reduced to solid silver (Ag(s)), which means that Ag⁺(aq) is the oxidizing agent, as it accepts electrons.

Therefore, the correct identification is: Fe(s) is the reducing agent and Ag⁺(aq) is the oxidizing agent.