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Question:

On the basis of standard electrode potential of redox couples given below, find out which of the following is the strongest oxidizing agent. (E⁰ values: Fe³⁺|Fe²⁺ = +0.77V; I₂(s)|I⁻ = +0.54V; Cu²⁺ = +0.34V; Ag⁺|Ag = +0.80V)

Cu²⁺

Ag⁺

Fe³⁺

I₂(s)

Solution:

Higher the reduction potential, better is the oxidizing agent. Now, the reduction potential decreases in the order: Ag⁺|Ag (+0.80V) > Fe³⁺|Fe²⁺ (+0.77V) > I₂(s)|I⁻ (+0.54V) > Cu²⁺|Cu (+0.34V). Hence, Ag⁺ is the strongest oxidizing agent.