Sponsor Area

Electrochemistry

Question
CBSEENCH12006125

Represent the cell in which the following reaction takes place:
Mg(s) + 2Ag+ (0.0001 M) → Mg2+(0.130 m) + 2Ag(s)
Calculate its E(cell), if E°cell = 3.17 V.

Solution
The cell is
Mg(s) | Mg2+(aq) (0.130 M) || Ag+(aq) (0.0001 M) | Ag(s)
The Nernst equation is
E(cell) = E°cell-RT2FlnMg2+Ag+Ecell = 3.17 V - 0.059 Vnlog0.130(0.0001)2Ecell = 3.17 V - 0.059 Vn×7.114Ecell  = 3.17 V - 0.21 VEcell = +2.96 V.