The Nernst Equation at 25°C:
Ecell = cell potential under non-standard conditions
E°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).
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.
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