Calculate E_cell for the following electrochemical cell at 25°C.The standard cell potential,E°_cell,is 0.460 V. Cu(s) | Cu²⁺(aq,0.016 M) || Ag⁺(aq,0.11 M) | Ag(s)

Question

Quizplus · Accepted Answer

The Nernst equation is used to calculate the cell potential under non-standard conditions. The equation is: E = E° - (RT/nF) * ln(Q), where E° is the standard cell potential, R is the gas constant, T is the temperature in Kelvin, n is the number of moles of electrons transferred in the reaction, F is the Faraday constant, and Q is the reaction quotient. For this cell, E° = 0.460 V, n = 1 (both Cu to Cu^2+ and Ag^+ to Ag involve the transfer of 1 electron), T = 25°C = 298 K, R = 8.314 J/(mol·K), and F = 96485 C/mol. Q = [Cu^2+]/[Ag^+] = 0.016/0.11. Plugging these values into the Nernst equation and solving gives a value closest to 0.456 V, making choice A correct.

Calculate Ecell for the Following Electrochemical Cell at 25°C

Calculate E_cell for the Following Electrochemical Cell at 25°C