Problem: Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 degrees C.Sn(s) │ Sn2+ (aq, 0.022M) ║ Ag+ (aq, 2.7M) │Ag(s)Write the net cell equation. Phases are optional. do not include the concentrationsCalculate the following values at 25.0 C using standard potentials as needed.E°cell =Ecell =ΔG°rxn =ΔGrxn =

FREE Expert Solution

The Nernst Equation at 25°C:

Ecell = Eocell - (0.05916 Vn)logQ

Ecell = cell potential under non-standard conditions
cell = standard cell potential
n = number of e- transferred
Q= reaction quotient = [products]/[reactants] 


We have to determine the E°cell first and as well as the anode (oxidation) and cathode (reduction) in the concentration cell and the number of electrons transferred (n).


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Problem Details

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 degrees C.

Sn(s) │ Sn2+ (aq, 0.022M) ║ Ag+ (aq, 2.7M) │Ag(s)

Write the net cell equation. Phases are optional. do not include the concentrations

Calculate the following values at 25.0 C using standard potentials as needed.

cell =

Ecell =

ΔG°rxn =

ΔGrxn =

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