The cell potential of a redox reaction occurring in an electrochemical cell unde

Question

The cell potential of a redox reaction occurring in an electrochemical cell under any set of temperature and concentration conditions can be determined from the standard cell potential of the cell using the Nernst equation E = E degree - (RT/nF)ln Q where E is the cell potential of the cell, E degree is the standard cell potential of the cell, R is the gas constant, T is the temperature in kelvin, n is the moles of electrons transferred in the reaction, and Q is the reaction quotient. Use this relationship to answer the problem below. For the following oxidation-reduction reaction Cu^2+(aq) + Zn(s) rightarrow Cu(s) + zn^2+(aq) the standard cell potential is 1.10 V What is the actual cell potential of the cell if the temperature is 314 K, the Cu^2+ (aq) initial Cu^2+ concentration is 0.00104 M, and the initial Zn^2+ concentration is 0.0205 M?

Explanation / Answer

E = Eo - (RT/ nF) ln Q

By converting this natural logarithm to the base of 10 and substituting the values of Eo, R = 8.314 J/ mol .K , and T = 314 K , and trhe concentration of both the species ,

E = 1.10 - (8.314 x 314 / 2 x 96500) 2.303 log (0.0205) / (0.00104)

E = 1.06 V

So the actual cell potential will be 1.06 V

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