(See attached file for full problem description)
The Nernst equation is the most important equation in electrochemistry.
It is defined as follows:
is the standard reduction potential of the reaction
is the gas constant
is the temperature (in Kelvin)
is the number of moles of electrons transferred in the reaction
is Faraday's constant, , and
For the reaction above, calculate the potential if the reaction occurs at and the concentrations are as follows:
0.411 , 0.169 , 5.60×10−2 , 9.90
Please see the attached file.
N is the number of electrons involved ...
The solution provides detailed explanations and calculations for the problem.
Electrochemistry and the Nernst Equation
1.Consider the following cell at equilibrium:
Mg(s) / Mg+2 (0.01 M) // OH- (?) / Mg(OH)2 (s) / Mg (s)
Given: Mg+2 + 2e- ---> Mg(s) Eo = -2.360 V
Mg(OH)2 (s) + 2e- ---> Mg(s) + 2 OH- Eo = -2.690 V
a) Write each half-reaction and the net cell reaction. Find the standard net cell potential.
b) Find the pH of the right cell when the cell is at equilibrium.
c) Draw the cell, clearly mark all the components, and show the anode and the cathode, and the direction of the flow of electrons. Which side of the cell is the reduction taking place?