We are asked to find the emf of the given reaction. We will use the Nernst Equation to calculate the cell potential with the given conditions.
The Nernst Equation relates the concentrations of compounds and cell potential.
Ecell = cell potential under non-standard conditions
E°cell = standard cell potential
n = number of e- transferred
Q= reaction quotient = [products]/[reactants]
Let’s first determine how many electrons were transferred in the reaction:
A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on the following half-reaction:
AgCl(s) + e- → Ag(s) + Cl- (aq).
The two cell compartments have [Cl- ] = 1.51×10−2 M and [Cl- ] = 2.60 M , respectively.
What is the cell emf for the concentrations given?
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