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Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Ag+(aq) + Pb(s) → 2Ag(s) + Pb2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: _____ G° for this reaction would be _________ (greater or less)   than zero.

Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Ag+(aq) + Pb(s) → 2Ag(s) + Pb2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: _____ G° for this reaction would be _________ (greater or less)   than zero.

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
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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Use standard reduction potentials to calculate the equilibrium constant for the reaction:

2Ag+(aq) + Pb(s) → 2Ag(s) + Pb2+(aq)

Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.

Equilibrium constant: _____

G° for this reaction would be _________ (greater or less)   than zero.

 

Sometimes the base-10 logarithm is used and the substitution of 2.303 log for In is made. (2.303 × 0.0257 = 0.0592) Then, the equation for base-10 logs at 25 °C is: 0.0592 E° cell log K 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:Sometimes the base-10 logarithm is used and the substitution of 2.303 log for In is made. (2.303 × 0.0257 = 0.0592) Then, the equation for base-10 logs at 25 °C is: 0.0592 E° cell log K 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.
Relationship between E°cell and K The equilibrium constant for a cell reaction can be calculated from the standard cell voltage. The relationship between them is: RT E°. cell - In K nF where standard cell 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 K = equilibrium constant E° R %3D 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 molr'K! T = 298.15 K F 96,485 J V' mol"1 (8.314 J moll K)(298.15 K) RT = 0.0257 V F 96,485 J V' mol" and the equation with the potential in volts is: 0.0257 E° cell In K natural logarithm Previous Next
Transcribed Image Text:Relationship between E°cell and K The equilibrium constant for a cell reaction can be calculated from the standard cell voltage. The relationship between them is: RT E°. cell - In K nF where standard cell 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 K = equilibrium constant E° R %3D 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 molr'K! T = 298.15 K F 96,485 J V' mol"1 (8.314 J moll K)(298.15 K) RT = 0.0257 V F 96,485 J V' mol" and the equation with the potential in volts is: 0.0257 E° cell In K natural logarithm Previous Next
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