1. Tardigrade
  2. Question
  3. Chemistry
  4. The more positive the value of E°, the greater is the tendency of the species to get reduced. Using the. standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent. E° values: Fe3+/Fe2+ = + 0.77; I2(s)/I- = + 0.54; Cu2+/Cu = + 0.34; Ag+/Ag = + 0.80 V

Question Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

Q. The more positive the value of $E^{\circ}$, the greater is the tendency of the species to get reduced. Using the. standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.
$E^{\circ}$ values : $Fe^{3+}/Fe^{2+} = + 0.77; I_{2\left(s\right)}/I^- = + 0.54$;
$Cu^{2+}/Cu = + 0.34$; $Ag^{+}/Ag = + 0.80\, V$

Redox Reactions

Solution:

Strongest oxidising agent means it has greater tendency to get reduced. Thus, $Ag^+$ having more positive $E^{\circ}$ value, is the strongest oxidising agent.