E° values of some redox couples are given below. On the basis of these values choose the correct option.
E° values: Br₂/Br^- = 1.09; Ag⁺ / Ag(s) = 0.80

Cu²⁺ /Cu(s) = + 0.34; I₂(s) /I = + 0.54

Question

E° values of some redox couples are given below. On the basis of these values choose the correct option. E° values: Br 2 /Br - = 1.09; Ag + / Ag(s) = 0.80 Cu 2+ /Cu(s) = + 0.34; I 2 (s) /I = + 0.54

Philoid · Accepted Answer

Reducing agents should have the ability to undergo oxidation that implies the property to easily loose electrons. Consequently the coupling element should have a greater tendency to attract the donated electron. As I^- and Br^- already are reduced ions so they cannot further undergo reduction. Between Ag and Br we can find from electrochemical series that the reduction potential of Br₂ is more as compared to Ag.

Thus Cu will reduce Br₂ as follows:

Corresponding [potential for the developed cell is

Thus Cu will reduce Br₂ as follows:

Corresponding [potential for the developed cell is

E° values of some redox couples are given below. On the basis of these values choose the correct option.E° values: Br2/Br- = 1.09; Ag+ / Ag(s) = 0.80Cu2+ /Cu(s) = + 0.34; I2(s) /I = + 0.54

E° values of some redox couples are given below. On the basis of these values choose the correct option.
E° values: Br₂/Br^- = 1.09; Ag⁺ / Ag(s) = 0.80

Cu²⁺ /Cu(s) = + 0.34; I₂(s) /I = + 0.54