Calculate the standard electrode potential difference (e°) of the daniell cell (at 1 bar) if temperature is 473.15 k.

Missing data in the text of the exercise: The molar concentration of Zinc is 10 times the molar concentration of copper.

Solution:

1) First of all, let's calculate the standard electrode potential difference at standard temperature. This is given by:

where  is the standard potential at the cathode, while  is the standard potential at the anode. For a Daniel Cell, at the cathode we have copper: , while at the anode we have zinc: . Therefore, at standard temperature the electrode potential difference of the Daniel Cell is


2) To calculate  at any temperature T, we should use Nerst equation:

where 

is the temperature in our problem
is the number of electrons transferred in the cell's reaction
is the Faraday's constant
and  are the molar concentrations of zinc and in copper, and in our problem we have .
Using all these data inside the equation, and using , in the end we find: