A concentration cell contains electrodes made of the same metal and solutions co
ID: 800570 • Letter: A
Question
A concentration cell contains electrodes made of the same metal and solutions containing the same ions but at different concentrations. Consider Zn electrode in 0.1 M ZnSO4 solution in one compartment and Zn electrode in 1.0 M ZnSO4 for another compartment of the cell. Write down the text diagram (form) for the cell and calculate the E for that cell at T=298K.
PLEASE SHOW HOW TO DO THE NERNST EQUATION FOR CALCULATING E.
A concentration cell contains electrodes made of the same metal and solutions containing the same ions but at different concentrations. Consider Zn electrode in 0.1 M ZnSO4 solution in one compartment and Zn electrode in 1.0 M ZnSO4 for another compartment of the cell. Write down the text diagram (form) for the cell and calculate the E for that cell at T=298K.Explanation / Answer
The cell notation is:
Zn(s) | Zn2+(aq, 0.1 M) || Zn2+(aq, 1.0 M) | Zn(s)
Overall cell reaction is:
Zn2+(aq, 1.0 M) => Zn2+(aq, 0.1 M)
Eo(cell) = 0.00 V
Moles of electrons transferred n = 2
Faraday constant F = 96485 C/mol
Molar gas constant R = 8.314 J/mol.K
Temperature T = 298 K
Nernst equation:
E(cell) = Eo(cell) - RT/nF ln([Zn2+(aq, 0.1 M]/[Zn2+(aq), 1.0 M)])
= 0.00 - 8.314 x 298/(2 x 96485) x ln(0.1/1.0)
= 0.0296 V (or approximately 0.030 V)
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