When writing a cell notation, we use the following format – “* as easy as ABC*”

Hence, the ** Cu/Cu^{+2} is the anode** reaction while

**(1) Calculating E° _{cell}**

$\overline{){\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cathode}}}{\mathbf{-}}{\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{anode}}}}$

**E°cell = 0.08 – (0.34)**

**E° _{cell} **= +0.46 V

(2) Calculating Ecell using Nernst equation:

$\overline{){{\mathbf{E}}}_{{\mathbf{cell}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}{\mathbf{-}}\frac{\mathbf{0}\mathbf{.}\mathbf{0591}}{\mathbf{2}}{\mathbf{log}}\frac{\left[{\mathrm{Cu}}^{+2}\right]}{{\mathbf{\left[}{\mathbf{Ag}}^{\mathbf{+}}\mathbf{\right]}}^{\mathbf{2}}}}\phantom{\rule{0ex}{0ex}}{\mathbf{E}}_{{\mathbf{cell}}}\mathbf{}\mathbf{=}\mathbf{}\mathbf{0}\mathbf{.}\mathbf{46}\mathbf{-}\frac{\mathbf{0}\mathbf{.}\mathbf{0591}}{\mathbf{2}}\mathbf{log}\frac{0.015}{{(2.5)}^{\mathbf{2}}}$

E_{cell }= +0.53 V

For the following electrochemical cell:

Cu(s)/Cu^^{2+}(aq,0.0155M//Ag^{+}(aq,2.50M)/Ag(s)

Write the net cell equation. Phases are optional. No not include concentrations.

Calculate the following values at 25 °C using standard potentials as needed:

Ecell(standard) = ____ v

Ecell = ____v

Δ G°rxn standard= kJ/mol

Δ G°rxn = kJ/mol

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Nernst Equation concept. You can view video lessons to learn The Nernst Equation. Or if you need more The Nernst Equation practice, you can also practice The Nernst Equation practice problems.