Chemistry - Electrochemistry Question with Solution | TestHub

For the strongest oxidizing agent, the oxidizing potential should be least. Here, the oxidizing potential of ${\mathrm{Fe}}^{+2}$ is less than that of ${\left[\mathrm{Fe}(\mathrm{CN}{)}_6\right]}^{4-}$. Therefore, ${\mathrm{Fe}}^{+2}$ is stronger oxidizing agent than ${\left[\mathrm{Fe}(\mathrm{CN}{)}_6\right]}^{4-}$. Also, the stronger oxidizing agent should easily reduce itself. Here, ${\mathrm{Fe}}^{+3}$ is easily reduced than ${\mathrm{Fe}}^{+2}$. Therefore, among all the four, ${\mathrm{Fe}}^{+3}$ is the stronger oxidizing agent.