Question

Calculate the potential for each cell as shown below and indicate whether the metal electrode in the half-reaction opposite the standard hydrogen electrode, s.h.e., would be the anode or the cathode if the cell was shorted and electrons were allowed to flow freely at 25 °c.
a.s.h.e. || zn2 (aq, 0.0250 m) | zn(s)

Answer 1

.086567 is what I think as being a math matichian

Answer 2

The cell voltage form the information provided in the question is 0.81 V.

The overall equation of the redox reaction that occurs in the two half cells is;

2H^+(aq) + Zn(s) ------> Zn^2+(aq) + H2(g)

Two electrons are transferred in the process so n =2

The standard hydrogen electrode involves hydrogen gas at 1 atm and hydrogen ion at 1 M.

Using the Nernst equation;

Ecell = E°cell - 0.0592/n logQ

Note that;

E°cell = 0.00 V - (-0.76 V) = 0.76 V

n = 2

Q = 0.0250 M/(1 M)^2 =  0.0250

So,

Ecell =  0.76 V - 0.0592/2 log(0.0250)

Ecell = 0.81 V

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