Final answer:
To calculate the cell potential (Ecell) for the reaction at 25°C with the given ion concentrations, we use the Nernst equation and find that Ecell is 1.59026 V.
Step-by-step explanation:
To calculate the cell potential (Ecell) of a galvanic cell at 25°C (298 K) for a given reaction with known concentrations of Ag+ and Zn2+ ions, we use the Nernst equation:
Ecell = E°cell - (0.0591/n) * log Q
Where E°cell is the standard electrode potential, n is the number of moles of electrons transferred in the reaction, and Q is the reaction quotient. For the reaction involving Ag+ and Zn2+, the E°cell value would be found from a standard electrode potentials table which typically contains values for Ag+/Ag and Zn2+/Zn half-cells.
If we assume the pair Ag+/Ag and Zn2+/Zn for our reaction, and know that the standard electrode potentials (E°) are 0.80 V for Ag+/Ag and -0.76 V for Zn2+/Zn, we then calculate E°cell for the cell:
E°cell = E°(Ag+/Ag) - E°(Zn2+/Zn)
E°cell = 0.80 V - (-0.76 V)
E°cell = 1.56 V
Now we can use the Nernst equation to find Ecell at non-standard conditions:
Ecell = 1.56 V - (0.0591/2) * log(0.066/0.697)
Ecell = 1.56 V - (0.0591/2) * log(0.0947)
Ecell = 1.56 V - 0.02955 * (-1.02398)
Ecell = 1.56 V + 0.03026 V
Ecell = 1.59026 V
The resulting Ecell at 25°C with the given ion concentrations of Ag+ and Zn2+ would be 1.59026 V, which indicates that the reaction should proceed spontaneously.