The equilibrium constant, K, for a redox reaction is related to the standard cell potential, E by the equation Standard reduction potentials In K Reduction half-reaction E° (V) where n is the number of moles of electrons transferred, F (the Faraday's constant) is equal to 06 500 C mol, R (the gas constant) is equal to 8.314 JK'mol, and Tis the Kelvin temperature. Ag' (aq) +e+Ag(a) Cu" (ag) + 2e Cu(s) Sn* (ag) + de-+Sn(s) 0.80 0.34 0.15 2H' (ag) + 2e-H3(9) N (ag) + 20-Ni(a) -0.26 Fe (ag) + 2eFe(a) -0.45 Zn" (ag) + 20-»Zn(s) -0.76 AB (ag) + 30 -+Al(s) -1.00 Mg* (aq) + 20 –→Mg(s) -2.37 • Part A 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) + N* (ag)-→F¢²*(aq) + Ni(o) Express your answer numerically. View Available Hint(s) Templates Symbol undo redo feset keyboard shortcuts Help
The equilibrium constant, K, for a redox reaction is related to the standard cell potential, E by the equation Standard reduction potentials In K Reduction half-reaction E° (V) where n is the number of moles of electrons transferred, F (the Faraday's constant) is equal to 06 500 C mol, R (the gas constant) is equal to 8.314 JK'mol, and Tis the Kelvin temperature. Ag' (aq) +e+Ag(a) Cu" (ag) + 2e Cu(s) Sn* (ag) + de-+Sn(s) 0.80 0.34 0.15 2H' (ag) + 2e-H3(9) N (ag) + 20-Ni(a) -0.26 Fe (ag) + 2eFe(a) -0.45 Zn" (ag) + 20-»Zn(s) -0.76 AB (ag) + 30 -+Al(s) -1.00 Mg* (aq) + 20 –→Mg(s) -2.37 • Part A 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) + N* (ag)-→F¢²*(aq) + Ni(o) Express your answer numerically. View Available Hint(s) Templates Symbol undo redo feset keyboard shortcuts Help
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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![Part B
Calculate the standard cell potential (E) for the reaction
X(s) + Y*(ag) = X*(ag) + Y(s)
if K = 2.03 x 10
Express your answer to three significant figures and include the appropriate units.
> View Available Hint(s)
Pesat
Tempjates Symbols undo redo fesél keyboard shortcuts Help
Value
Units
"cell](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffe89836b-bba0-4df5-9667-e99956de1c6d%2F2d68c838-623b-4c21-8269-76f8f77ba946%2F0fcv7d5_processed.png&w=3840&q=75)
Transcribed Image Text:Part B
Calculate the standard cell potential (E) for the reaction
X(s) + Y*(ag) = X*(ag) + Y(s)
if K = 2.03 x 10
Express your answer to three significant figures and include the appropriate units.
> View Available Hint(s)
Pesat
Tempjates Symbols undo redo fesél keyboard shortcuts Help
Value
Units
"cell
![The equilibrium constant, K, for a redox reaction is related to the standard cell potential, E.
by the equation
Standard reduction potentials
In K
Reduction half-reaction E (V)
Ag (ag) +e
where n is the number of moles of electrons transferred, F (the Faraday's constant) is equal to
98 500 C mol-. R (the gas constant) is equal to 8.314JK
temperature.
+Ag(s)
0.80
and T is the Kelvin
Cu2+ (ag) + 2e-Cu(s)
0.34
Sn+ (ag) + de-→Sn(s)
0.15
2H*(ag) + 2e+H2(g)
Ni+ (ag) + 2e-→Ni(s)
-0.26
Fe2+ (ag) + 20FE(s)
-0.45
Zn2+ (ag) + 2e-+Zn(s)
-0.78
Al3+ (ag) + 3e +Al(s)
-1.66
Mg+ (ag) + 2e →Mg(s) -2.37
• Part A
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) + Ni*+ (ag)→Fe* (ag) + Ni(s)
Express your answer numerically.
> View Available Hint(s)
Templates SymBols undo rego fese keyboard shortcuts help
K =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffe89836b-bba0-4df5-9667-e99956de1c6d%2F2d68c838-623b-4c21-8269-76f8f77ba946%2Fgim0trq_processed.png&w=3840&q=75)
Transcribed Image Text:The equilibrium constant, K, for a redox reaction is related to the standard cell potential, E.
by the equation
Standard reduction potentials
In K
Reduction half-reaction E (V)
Ag (ag) +e
where n is the number of moles of electrons transferred, F (the Faraday's constant) is equal to
98 500 C mol-. R (the gas constant) is equal to 8.314JK
temperature.
+Ag(s)
0.80
and T is the Kelvin
Cu2+ (ag) + 2e-Cu(s)
0.34
Sn+ (ag) + de-→Sn(s)
0.15
2H*(ag) + 2e+H2(g)
Ni+ (ag) + 2e-→Ni(s)
-0.26
Fe2+ (ag) + 20FE(s)
-0.45
Zn2+ (ag) + 2e-+Zn(s)
-0.78
Al3+ (ag) + 3e +Al(s)
-1.66
Mg+ (ag) + 2e →Mg(s) -2.37
• Part A
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) + Ni*+ (ag)→Fe* (ag) + Ni(s)
Express your answer numerically.
> View Available Hint(s)
Templates SymBols undo rego fese keyboard shortcuts help
K =
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