The potential of this cell is 1.53 volts, so the correct answer is A. 1.53 volts.
To find the potential of the cell using the Nernst equation, we can use the formula E= E^∘- (2.303RT)/(nF) log Q, where E° is the standard cell potential, R is the gas constant (8.314 J/(mol·K)), T is the temperature in Kelvin, n is the number of moles of electrons transferred in the balanced chemical equation, F is Faraday's constant (96,485 C/mol), and Q is the reaction quotient.
Plugging in the given values:
E° = +1.56 volts
T = 100°C = 373 K
[Ag+] = 5.0 M
[Zn2+] = 1.0 M
The balanced chemical equation shows that 2 moles of electrons are transferred, so n = 2.
Using the Nernst equation, we can calculate:
E= 1.56 - ((2.303 * 8.314 * 373)/(2 * 96485)) * log(5.0^2 / 1.0)
E= 1.56 - (4.551 * 10^-3) * log(25)
E= 1.56 - (4.551 * 10^-3) * 1.397
E= 1.56 - 6.35 * 10^-3
E= 1.53 volts
Therefore, the potential of this cell is 1.53 volts, so the correct answer is A. 1.53 volts.