Standard electrode potentials for a few half cells are mentioned below: E°_ Cu²⁺/Cu = 0.34 V, E°_ Zn²⁺/Zn = -0.76 V, E° Ag⁺/Ag = 0.80 V, E°_ Mg²⁺/Mg = -2.37 V. Which one of the following cells gives the most negative value of Δ G° ?

(C) Zn|Zn²⁺(1M)||Ag⁺(1M)|Ag

(A) Zn|Zn²⁺(1M)||Mg²⁺(1M)|Mg

(B) Cu|Cu²⁺(1M)||Ag⁺(1M)|Ag

(D) Ag|Ag⁺(1M)||Mg²⁺(1M)|Mg

Redox Reactions and Electrochemistry: JEE Main 2025 Chemistry question

JEE Main 2025 · 23 Jan, Evening shift · Q56

JEE Main 202523 Jan, Evening shiftChemistryMediumRedox Reactions and Electrochemistry138× since 2002

Standard electrode potentials for a few half cells are mentioned below:

E^\circ_{\mathrm{Cu^{2+}/Cu}} = 0.34

E^\circ_{\mathrm{Zn^{2+}/Zn}} = -0.76

E^\circ_{\mathrm{Ag^+/Ag}} = 0.80

E^\circ_{\mathrm{Mg^{2+}/Mg}} = -2.37

V. Which one of the following cells gives the most negative value of

\Delta G^\circ

JEE Main 2025 · 23 Jan, Evening shift · Q56

JEE Main 202523 Jan, Evening shiftChemistryMediumRedox Reactions and Electrochemistry138× since 2002

Standard electrode potentials for a few half cells are mentioned below:

E^\circ_{\mathrm{Cu^{2+}/Cu}} = 0.34

E^\circ_{\mathrm{Zn^{2+}/Zn}} = -0.76

E^\circ_{\mathrm{Ag^+/Ag}} = 0.80

E^\circ_{\mathrm{Mg^{2+}/Mg}} = -2.37

V. Which one of the following cells gives the most negative value of

\Delta G^\circ