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

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 (A) Fe3+ (B) I2(s) (C) Cu2+ (D) Ag+

Tardigrade Admin · Accepted Answer

Strongest oxidising agent means it has greater tendency to get reduced. Thus, Ag+ having more positive E° value, is the strongest oxidising agent.

$F e^{3 +}$

$I_{2 (s)}$

$C u^{2 +}$

$A g^{+}$

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

Fe3+

I2(s)​

Cu2+

Ag+

Strongest oxidising agent means it has greater tendency to get reduced. Thus, Ag+ having more positive E∘ value, is the strongest oxidising agent.

$F e^{3 +}$

$I_{2 (s)}$

$C u^{2 +}$

$A g^{+}$

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