t The Nernst Equation The Nernst equation is one of the most important equations

Question

t The Nernst Equation The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is 2.303 RT nF where E is the potential in volts, E s the standard potential in volts, R is the gas constant T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q is the reaction quotient. At standard temperature, 25 C or 298 K, the equation has the form o 0.0592 log O The reaction quotient has the usual form products reactants A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure Part A For the reaction 2Co3 (aq) 2 Cl (aq) 2Co2+ (aq) Cl2(g). EP 0.71 V what is the cell potential at 25 o C if the concentrations are Co 3.40x10-2M. Co2+ 0.403 M and Cl 0.106M and the pressure of Cl2 is PC 3.80 atm Express your answer with the appropriate units. LLA E. alue Units Submit Hints My Answers Give Up Review Part Continue Provide Feedback

Explanation / Answer

Given data

Eo = 0.71 V

[Co3+] = 3.40*10-2 M

[Co2+]= 0.403 M

[Cl-] = 0.106 M

P[Cl2] = 3.80 atm

E = ?

Formula to calculate cell potential is as follows

E= Eo - (0.0592/n) * log Q

Q = [product]x/[reactant]y

So equation becomes

E= Eo - (0.0592/n) * log ([Co2+]2[Cl2])/([ Co3+]2[ Cl-]2)

Lets put the values in the formula and calculate E

Here n = 2 because 2 electrons transferred

E = 0.71 V

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

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