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What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 3.59×10-4 M and the Cr3+ concentration is 1.07 M ? 3Hg2+(aq) + 2Cr(s) →3Hg(l) + 2Cr3+(aq) Answer:  ____ V The cell reaction as written above is spontaneous for the concentrations given: _______ (true or false)

What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 3.59×10-4 M and the Cr3+ concentration is 1.07 M ? 3Hg2+(aq) + 2Cr(s) →3Hg(l) + 2Cr3+(aq) Answer:  ____ V The cell reaction as written above is spontaneous for the concentrations given: _______ (true or false)

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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What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 3.59×10-4 M and the Cr3+ concentration is 1.07 M ?

3Hg2+(aq) + 2Cr(s) →3Hg(l) + 2Cr3+(aq)

Answer:  ____ V

The cell reaction as written above is spontaneous for the concentrations given: _______ (true or false)
 
The Nernst Equation A non-standard cell or half-cell potential can be calculated using the Nernst Equation: RT E = E° - . In Q nF where E = potential under non-standard conditions standard potential = ideal gas constant T = kelvin temperature n = number of moles of electrons for the reaction as written F = charge carried by 1 mol of electrons Q = reaction quotient E° R It is customary to use the equation in a form where numerical values are substituted for R, T and F at a temperature of 25 °C. For R = 8.314 J mol'K! T = 298.15 K 96,485 J V-l mol" F = (8.314 J mol! K(298.15 K) RT = 0.0257 V F 96,485 J V-' mol-1 and the Nernst equation with the potentials in volts is: Previous 0.0257 In 0 Hatural lagarithn.
Transcribed Image Text:The Nernst Equation A non-standard cell or half-cell potential can be calculated using the Nernst Equation: RT E = E° - . In Q nF where E = potential under non-standard conditions standard potential = ideal gas constant T = kelvin temperature n = number of moles of electrons for the reaction as written F = charge carried by 1 mol of electrons Q = reaction quotient E° R It is customary to use the equation in a form where numerical values are substituted for R, T and F at a temperature of 25 °C. For R = 8.314 J mol'K! T = 298.15 K 96,485 J V-l mol" F = (8.314 J mol! K(298.15 K) RT = 0.0257 V F 96,485 J V-' mol-1 and the Nernst equation with the potentials in volts is: Previous 0.0257 In 0 Hatural lagarithn.
and the Nernst equation with the potentials in volts is: 0.0257 E = E° In Q natural logarithm Sometimes it is more convenient to use base-10 logarithms and the substitution of 2.303 log for In is made. (2.303 x 0.0257 = 0.0592) Then, the Nernst equation for base-10 logs at 25 °C is: 0.0592 E = E° log Q base-10 logarithm n A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm.
Transcribed Image Text:and the Nernst equation with the potentials in volts is: 0.0257 E = E° In Q natural logarithm Sometimes it is more convenient to use base-10 logarithms and the substitution of 2.303 log for In is made. (2.303 x 0.0257 = 0.0592) Then, the Nernst equation for base-10 logs at 25 °C is: 0.0592 E = E° log Q base-10 logarithm n A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm.
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