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A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm. Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: Ni2+ (aq) + Cu(s) Ni(s) + Cu+ (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 be v than zero. greater less Retry Entire Grd Submit Answer bre arnun attemnte remaininn

A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm. Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: Ni2+ (aq) + Cu(s) Ni(s) + Cu+ (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 be v than zero. greater less Retry Entire Grd Submit Answer bre arnun attemnte remaininn

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 31E: Determine the standard cell potential and the cell potential under the stated conditions for the...
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The Nernst Equation A nonstandard cell or half-cell potential can be calculated using the Nernst equation: RT E = E°- InQ %3D nF 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 %3D Q = 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 and the Nernst equation with the potentials in volts is: 0.02568 In Q E = E° - n 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 E = E 0.0591 logQ A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm. Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: Ni²+ (aq) + Cu(s) → Ni(s) + Cu²+ (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. K = %3D AG° for this reaction would be than zero. greater less Retry Entire Gre Submit Answer bre aroun attemnts remainina
Transcribed Image Text:The Nernst Equation A nonstandard cell or half-cell potential can be calculated using the Nernst equation: RT E = E°- InQ %3D nF 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 %3D Q = 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 and the Nernst equation with the potentials in volts is: 0.02568 In Q E = E° - n 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 E = E 0.0591 logQ A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm. Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: Ni²+ (aq) + Cu(s) → Ni(s) + Cu²+ (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. K = %3D AG° for this reaction would be than zero. greater less Retry Entire Gre Submit Answer bre aroun attemnts remainina
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