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/n F)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 initial Cu^2+ concentration is 0.00104 M, and the initial zn^2+ concentration is 0.0205 M? (Note that the reaction involves the transfer of 2 moles of electrons, and the reaction quotient is 19.7.) V

Explanation / Answer

E = E° - RT/(nF)*ln(Q)

n = 2 electrons

Q = [Zn+2]/[Cu+2] = 0.0205 / 0.00104 = 19.711

R = 8.314, T = 314 K, E° = 1.10

E = E° - RT/(nF)*ln(Q)

E = 1.1 - 8.314*314/(2*96500)*ln(19.711)

E = 1.05967 V

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.