The Nernst EquationA nonstandard cell or half-cell potential can be calculated using the Nernst equation:RTInQnFE = E°-whereE = potential under nonstandard conditions%3DE = standard potentialR = ideal gas constant = 8.314 J/K mol%3DT = kelvin temperaturen = number of moles of electrons for the reaction aswrittenF = charge carried by 1 mol of electrons =%3D96, 485 C/mol = 96, 485 J/V mol%3DQ = reaction quotient%3DIt is customary to use the equation in a form where numberical values are substituted for R, T, and F at a temperature of 25°C.(8.314 J/K mol)(298K)96, 485 J/V molRT= 0.02568 V%3Dand the Nernst equation with the potentials in volts is:0.02568In QE = E -nSometimes it is more convenient to use base-10 logarithms, and the substitution of 2.3026 log for In is made.(2.3026 x 0.02568 =0.0591)%3D0.0591logQE = E° –A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correctlogarithm.Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction:2Cu2+ (aq) + Sn(s) 2Cu* (aq) + Sn2+ (aq)Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.K =AG° for this reaction would bethan zero.greaterlessRetry Entire GreSubmit AnswerJare groun attemnts remaining

A nonstandard cell or half-cell potential can be calculated using the Nernst equation: RT InQ nF E= E -- where E = potential under nonstandard conditions %3D E = standard potential R = ideal gas constant = 8.314 J/K mol %3D T = kelvin temperature %3D n = number of moles of electrons for the reaction as written F = charge carried by 1 mol of electrons = 96, 485 C/mol = 96, 485 J/V mol %3D

A nonstandard cell or half-cell potential can be calculated using the Nernst equation: RT InQ nF E= E -- where E = potential under nonstandard conditions %3D E = standard potential R = ideal gas constant = 8.314 J/K mol %3D T = kelvin temperature %3D n = number of moles of electrons for the reaction as written F = charge carried by 1 mol of electrons = 96, 485 C/mol = 96, 485 J/V mol %3D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The Nernst Equation. A nonstandard cell or half-cell potential can be calculated using the Nernst equation: RT InQ nF E = E %3D where E = potential under nonstandard conditions %3D E = standard potential R = ideal gas constant = 8.314 J/K mol %3D T = kelvin temperature 2%3= number of moles of electrons for the reaction as written F = charge carried by 1 mol of electrons = 96, 485 C/mol = 96, 485 J/V mol %3D = reaction quotient %3D It is customary to use the equation in a form where numberical values are substituted for R, T, and F at a temperature of 25°C. (8.314 J/K mol)(298K) 96, 485 J/V mol RT = 0.02568 V F and the Nernst equation with the potentials in volts is: 0.02568 In Q E = E - Sometimes it is more convenient to use base-10 logarithms, and the substitution of 2.3026 log for In is made. (2.3026 x 0.02568 = 0.0591) %3D 0.0591 logQ E = E - A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm. What is the…
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