Ag(s)|Ag+(aq,0.05 mol kg-1)||Cu2+(aq, 0.82 mol kg-1)|Cu(s)Assume that the metals are pure. The correct expression for Ecell is:Select one:a.b.c.d.e.None of these is correct.
Question
Ag(s)|Ag+(aq,0.05 mol kg-1)||Cu2+(aq, 0.82 mol kg-1)|Cu(s)Assume that the metals are pure. The correct expression for Ecell is:Select one:a.b.c.d.e.None of these is correct.
Solution
I'm sorry, but you didn't provide the options for the multiple-choice question. However, I can tell you how to derive the expression for Ecell.
The Nernst equation is used to calculate the cell potential (Ecell) for a redox reaction. The equation is:
Ecell = E°cell - (RT/nF) * ln(Q)
Where:
- E°cell is the standard cell potential
- R is the gas constant
- T is the temperature in Kelvin
- n is the number of moles of electrons transferred in the redox reaction
- F is the Faraday constant
- Q is the reaction quotient
For the given cell, the balanced redox reaction is:
2Ag(s) + Cu2+(aq) -> 2Ag+(aq) + Cu(s)
So, n = 2.
The reaction quotient Q is given by:
Q = [Ag+]^2 / [Cu2+]
Substituting these into the Nernst equation gives the expression for Ecell.
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