What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu+ concentration is 1.07 M and the Al* concentration is 7.70 x 10 M? 3Cu" (aq) + 2AI(s) + 3Cu(s) + 2A1* (aq) Ecell =| The cell reaction as written above is for the concentrations given. spontaneous nonspontaneous www r pts remaining Submit Answer Retry Entire Group
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu+ concentration is 1.07 M and the Al* concentration is 7.70 x 10 M? 3Cu" (aq) + 2AI(s) + 3Cu(s) + 2A1* (aq) Ecell =| The cell reaction as written above is for the concentrations given. spontaneous nonspontaneous www r pts remaining Submit Answer Retry Entire Group
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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![The Nernst Equation
A nonstandard cell or half-cell potential can be calculated using the Nernst equation:
RT
E = E-
InQ
nF
where
E = potential under nonstandard conditions
E = standard potential
R = ideal gas constant 8.314 J/K mol
%3D
%3D
T = kelvin temperature
n = number of moles of electrons for the reaction as
written
%3D
F = charge carried by 1 mol of electrons =
96, 485 C/mol = 96, 485 J/V · mol
%3D
%3D
= 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.
RT (8.314 J/K - mol)(298K)
96, 485 J/V mol
= 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)
E = E° –
0.0591
logQ
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 298K for an electrochemical cell with the following reaction, when the Cu+
concentration is 1.07 M and the Al* concentration is 7.70 × 10¬ M ?
3Cu+ (aq) + 2Al(s) → 3Cu(s) + 2Al* (aq)
Ecel
V
The cell reaction as written above is
v for the concentrations given.
spontaneous
nonspontaneous
Submit Answer
Retry Entire Group
pts remaining](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff70653cf-152a-4edf-8c62-be28491f21e3%2Fa34cae30-692f-49ce-b09e-06e17349a90e%2Ff86mise_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The Nernst Equation
A nonstandard cell or half-cell potential can be calculated using the Nernst equation:
RT
E = E-
InQ
nF
where
E = potential under nonstandard conditions
E = standard potential
R = ideal gas constant 8.314 J/K mol
%3D
%3D
T = kelvin temperature
n = number of moles of electrons for the reaction as
written
%3D
F = charge carried by 1 mol of electrons =
96, 485 C/mol = 96, 485 J/V · mol
%3D
%3D
= 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.
RT (8.314 J/K - mol)(298K)
96, 485 J/V mol
= 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)
E = E° –
0.0591
logQ
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 298K for an electrochemical cell with the following reaction, when the Cu+
concentration is 1.07 M and the Al* concentration is 7.70 × 10¬ M ?
3Cu+ (aq) + 2Al(s) → 3Cu(s) + 2Al* (aq)
Ecel
V
The cell reaction as written above is
v for the concentrations given.
spontaneous
nonspontaneous
Submit Answer
Retry Entire Group
pts remaining
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