Consider the following electrochemical cell: Cu | Cu (NO3) 2 (0.0500 M) || Zn (N

Question

Consider the following electrochemical cell: Cu | Cu (NO3) 2 (0.0500 M) || Zn (NO3) 2 (0.0500 M) | Zn

Using http://web.mst.edu/~gbert/Electro/Electrochem.html To assemble the electrochemical cell and compare the result obtained in the simulation with their calculations.

A. Taking into account the average reactions: Cu + 2 + 2e- Cu (s) E ° = +0.337 V Zn + 2 + 2e - Zn (s) E ° = -0.763 V Without making any kind of calculation, does the electrochemical cell of the form in which it is presented occur spontaneously?

B. Perform the assembly of the cell in the simulation. What is the potential registered?

C. Demonstrate the potential in a theoretical way (potential calculation).

Explanation / Answer

Cu(s) to Cu+2 and Zn+2 to Zn(s)

a)

For this to occurs spontanous, the Ecell must be possitive value

that is

Ecell = Ered - Eox, so

Ered > Eox always

then

the only value that will be true is Copper reducing and Zinc oxidzing. Therefore, this is NOT spontanous, since in the cell shown above, the reverse is ocurring

B)

For the potential:

Ecell = -1.102 V

c)

For the potential in the "theretical way"

Must be the inverted sign, since the concentrations are the same, n value is also 2 electrons flow so

Epotential for spontanoeous reaciton = 1.102 V

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