Question

Consider the following standard reduction potentials: Zn2+(aq) + 2 e− LaTeX: \longrightarrow⟶ Zn(s) Eo = −0.76 V Mg2+(aq) + 2 e− LaTeX: \longrightarrow⟶ Mg(s) Eo = −2.37 V Ag+(aq) + e− LaTeX: \longrightarrow⟶ Ag(s) Eo = +0.80 V Which is the strongest oxidizing agent? Group of answer choices

Answer 1

Answer: The strongest oxidizing agent is silver.

Explanation:

Oxidizing agents are defined as the agents which oxidize other substance and itself gets reduced. These agents undergoes reduction reactions and reduction reaction is the reaction in which an atom gains electrons.

The substance having highest positive reduction $E^o$ potential will always get reduced and will undergo reduction reaction easily.

We are given:

$Zn^{2+}(aq.)+2e^-\rightarrow Zn(s);E^o =-0.76V$

$Mg^{2+}(aq.)+2e^-\rightarrow Mg(s);E^o =-2.37V$

$Ag^{+}(aq.)+e^-\rightarrow Ag(s);E^o =+0.80V$

As, silver has the highest positive reduction potential. So, it will be the strongest oxidizing agent.

Hence, the strongest oxidizing agent is silver.