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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 where E = potential under nonstandard conditions E = standard potential R = ideal gas constant 8.314 J/K mol T = kelvin temperature 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 Q = reaction quotient 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 %3D F and the Nernst equation with the potentials in volts is: E = E° 0.02568 In Q 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) 0.0591 E = E - logQ 72 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 calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Cu+ concentration is 5.09 x 10 M and the Mg* concentration is 1.33 M ? Cu+ (aq) + Mg(s) → Cu(s) + Mg+ (aq) Ecell V The cell reaction as written above is v for the concentrations given. spontaneous Submit Answer Retry Entire Group nonspontaneous pts remaining

The Nernst Equation A nonstandard cell or half-cell potential can be calculated using the Nernst equation: RT E= E - InQ where E = potential under nonstandard conditions E = standard potential R = ideal gas constant 8.314 J/K mol T = kelvin temperature 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 Q = reaction quotient 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 %3D F and the Nernst equation with the potentials in volts is: E = E° 0.02568 In Q 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) 0.0591 E = E - logQ 72 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 calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Cu+ concentration is 5.09 x 10 M and the Mg* concentration is 1.33 M ? Cu+ (aq) + Mg(s) → Cu(s) + Mg+ (aq) Ecell V The cell reaction as written above is v for the concentrations given. spontaneous Submit Answer Retry Entire Group nonspontaneous pts remaining

Chemistry
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
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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 calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Cu+ concentration is 5.09 × 10~ M and the Mg²+ concentration is 1.33 M ? Cu* (aq) + Mg(s) → Cu(s) + Mg²+ (aq) Ecll V The cell reaction as written above is for the concentrations given. spontaneous nonspontaneous Submit Answer Retry Entire Group pts remaining
Transcribed Image Text: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 calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Cu+ concentration is 5.09 × 10~ M and the Mg²+ concentration is 1.33 M ? Cu* (aq) + Mg(s) → Cu(s) + Mg²+ (aq) Ecll V The cell reaction as written above is for the concentrations given. spontaneous nonspontaneous Submit Answer Retry Entire Group pts remaining
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