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 = Eo- 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 RT nF In here E is the cell potential of the cell Eo is the standard cell potential of the cell, R is For the following oxidation-reduction reaction 2 Au3+(aq) + 3 Cu(s) 2 Au(s) + 3 Cu2+(aq) the standard cell potential is 1.16 V. What is the actual cell potential of the cell if the temperature is 320 K, the initial Au3+coenration is o.00108 M, and the initial Cu2+ concentration is o.0246 M? (Note that the reaction involves the transfer of 6 moles of electrons, and the reaction quotient is 12.8.)

Explanation / Answer

E(cell) = E(standard) - RT/nF(Q) (this formula is given )

at first we find the reaction quotient =

2 Au(3+)(aq) + 3 Cu(s)-----------------> 2 Au(s) + 3Cu(2+)

Q= [[Au]^2*[Cu(2+)]^3]/[[Cu]^3*[Au(3+)]^2]

we all know for solid substance put 1 .

now Q= [Cu(2+)]^3/[Au(3+)]^2

putiing the values .

Q= [0.0246]^3/[0.0018]^2

Q= 12.7631 which is equal to given Q = 12.8 value in the question .

now for cell equation

E = E* -RT/nFln(Q) E* =1.16V , R=8.314 ,T= 320 K , n=6 , F=96487

E= 1.16 - 8.314*320/6*96487[ln(12.8)]

E = 1.16- 0.0117

E = 1.1483.V

most confusing thing is here that the concentration of ions as well as value of Q both is given here . but when we check the value of by given concentration it is same ..........

IF U SATISFY WITH THE SOLUTION PLEASE LIKE IT ........................THNKXXXXXXXXXXX

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

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