Calculate the standard cell potential in (V) of the cell in which the following reaction takes place: Fe^2+(aq) + Ag^+(aq) → Fe^3+(aq) + Ag(s). Given that E^o_Ag^+/Ag = xV, E^o_Fe^2+/Fe = yV, E^o_Fe^3+/Fe = zV

Correct option is A. x + 2y - 3z
Solution:- (A) x + 2y - 3z
Fe^2+(aq) + Ag^+(aq) → Fe^3+ (aq) + Ag(s)
Cell reaction,
Anode: Fe^2+(aq) → Fe^3+ (aq) + e⁻; E^o_Fe^2+/Fe^3+ = mV
Cathode: Ag^+(aq) + e⁻ → Ag(s); E^o_Ag^+/Ag = xV
→ cell standard potential = (m + x)V
Now, to find 'm',
Fe^2++2e⁻ → Fe; E^o_1 = yV → ΔG_1^o = (2Fy)
Fe^3++3e⁻ → Fe; E^o_2 = zV → ΔG_2^o = (3Fy)
Fe^2+(aq) → Fe^3+(aq) + e⁻; E^o_3 = mV → ΔG_3^o = -(1Fm)
ΔG_3^o = ΔG^0_1 - ΔG^o_2 = (-2Fy + 3Fz) = -Fm
→ m = (2y - 3z)
→ E^o_cell = (x + 2y - 3z)V