The standard cell potential (e°cell) for the reaction below is +0.63 v. the cell potential for this reaction is when the concentration of zn2+ = 1.0 m and theconcentration of pb2+ = 2.0 x 10-4 m. pb2+(aq) + zn(s) > zn2+(aq) + pb(s) include details of how to calculate the need the steps. in advance.

The cell potential of the above reaction is 0.52 V

Explanation:

The given chemical equation follows:

Oxidation half reaction:  

Reduction half reaction:  

To calculate the EMF of the cell, we use the Nernst equation, which is:

where,

= electrode potential of the cell = ? V

= standard electrode potential of the cell = 0.63 V

n = number of electrons exchanged = 2

Putting values in above equation, we get:

Hence, the cell potential of the above reaction is 0.52 V

a:

by the combination of an unlimited number of elements