+ Cell Potential and Equilibrium The equilibrium constant, K. for a redox reaction is related to the standard potential, E, by the equation nFE RT In K where 11 is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96.500 C/(mol e). R (the gas constant) is equal to 8.314 J/(mol K), and T is the Kelvin temperature. Standard reduction potentials ▼ Part A Express your answer numerically. View Available Hint(s) K= IVE ΑΣΦ ] + Reduction half-reaction Ag (aq) +eAg(s) Cu²+ (aq) + 2e Sn (aq) + 4e Sn(s) 2H+ (aq) +2e →>H₂(g) ? Ni²+ (aq) + 2e Fe2+ (aq) +2e Zn²+ (aq) + 2e AP (aq) + 3e Mg2+ (aq) + 2e Cu(s) Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + Ni²+ (aq) >Fe²+ (aq) + Ni(s) E° (V) 0.80 0.34 0.15 0 -0.20 Ni(s) 0.45 Fe(s) Zn(s) Al(s) Mg(s) -2.37 0.76 -1.68 < 29 o Review Constants | Period
+ Cell Potential and Equilibrium The equilibrium constant, K. for a redox reaction is related to the standard potential, E, by the equation nFE RT In K where 11 is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96.500 C/(mol e). R (the gas constant) is equal to 8.314 J/(mol K), and T is the Kelvin temperature. Standard reduction potentials ▼ Part A Express your answer numerically. View Available Hint(s) K= IVE ΑΣΦ ] + Reduction half-reaction Ag (aq) +eAg(s) Cu²+ (aq) + 2e Sn (aq) + 4e Sn(s) 2H+ (aq) +2e →>H₂(g) ? Ni²+ (aq) + 2e Fe2+ (aq) +2e Zn²+ (aq) + 2e AP (aq) + 3e Mg2+ (aq) + 2e Cu(s) Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + Ni²+ (aq) >Fe²+ (aq) + Ni(s) E° (V) 0.80 0.34 0.15 0 -0.20 Ni(s) 0.45 Fe(s) Zn(s) Al(s) Mg(s) -2.37 0.76 -1.68 < 29 o Review Constants | Period
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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Question
![+ Cell Potential and Equilibrium
The equilibrium constant, K, for a redox reaction is related to the standard
potential, E, by the equation
In K FE
RT
where 72 is the number of moles of electrons transferred, F (the Faraday
constant) is equal to 96,500 C/(mol e-). R (the gas constant) is equal to
8.314 J/(mol K), and T is the Kelvin temperature.
Standard reduction potentials
▾ Part A
Use the table
Express your answer numerically.
▸ View Available Hint(s)
K=
ΥΠΙ ΑΣΦ 9
Reduction half-reaction
Ag+ (aq) +eAg(s)
Cu²+ (aq) +201
>Cu(s)
Sn+ (aq) + 4e →→Sn(s)
2H+ (aq) +2e →H₂(g)
Ni2+ (aq) + 2e →Ni(s)
Fe²+ (aq) + 2e →Fe(s)
Zn²+ (aq) +2e →Zn(s)
Al³+ (aq) + 3e →Al(s)
Mg²+ (aq) + 2e →Mg(s)
standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction:
Fe(s) + Ni²+ (aq) →>Fe²+ (aq) + Ni(s)
?
E (V)
0.80
0.34
0.15
0
0.26
-0.45
0.76
-1.66
2.37
29 o
Review | Constants | Period](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4f1d9a89-71fd-4cbf-9dfd-d06b2874d66e%2Ff533e901-6886-4e33-9c0b-ff2c9d372427%2Fr9hzn0k_processed.jpeg&w=3840&q=75)
Transcribed Image Text:+ Cell Potential and Equilibrium
The equilibrium constant, K, for a redox reaction is related to the standard
potential, E, by the equation
In K FE
RT
where 72 is the number of moles of electrons transferred, F (the Faraday
constant) is equal to 96,500 C/(mol e-). R (the gas constant) is equal to
8.314 J/(mol K), and T is the Kelvin temperature.
Standard reduction potentials
▾ Part A
Use the table
Express your answer numerically.
▸ View Available Hint(s)
K=
ΥΠΙ ΑΣΦ 9
Reduction half-reaction
Ag+ (aq) +eAg(s)
Cu²+ (aq) +201
>Cu(s)
Sn+ (aq) + 4e →→Sn(s)
2H+ (aq) +2e →H₂(g)
Ni2+ (aq) + 2e →Ni(s)
Fe²+ (aq) + 2e →Fe(s)
Zn²+ (aq) +2e →Zn(s)
Al³+ (aq) + 3e →Al(s)
Mg²+ (aq) + 2e →Mg(s)
standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction:
Fe(s) + Ni²+ (aq) →>Fe²+ (aq) + Ni(s)
?
E (V)
0.80
0.34
0.15
0
0.26
-0.45
0.76
-1.66
2.37
29 o
Review | Constants | Period
![Part B
Calculate the standard cell potential (E) for the reaction
if K = 8.82x10-³
Express your answer to three significant figures and include the appropriate units.
▸ View Available Hint(s)
Submit
Value
Units
X(s) +Y+ (aq) X+ (aq) +Y(s)
?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4f1d9a89-71fd-4cbf-9dfd-d06b2874d66e%2Ff533e901-6886-4e33-9c0b-ff2c9d372427%2Fsxlzk8p_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Part B
Calculate the standard cell potential (E) for the reaction
if K = 8.82x10-³
Express your answer to three significant figures and include the appropriate units.
▸ View Available Hint(s)
Submit
Value
Units
X(s) +Y+ (aq) X+ (aq) +Y(s)
?
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