Thank you! + Introduction to the Nernst EquationLearning Goal:To learn how to use the Nernst equation.The standard reduction potentials listed in any reference table are onlyvalid at the common reference temperature of 25 °C and standardconditions of 1 M for solutions and 1 atm for gases. To calculate thecell potential at nonstandard conditions, one uses the Nernst equation,2.303 RTE = EnF-log10 Qwhere E is the potential in volts, E is the standard potential at 25 °Cin volts, R = 8.314 J/(K-mol) is the gas constant, T is thetemperature in kelvins, n is the number of moles of electronstransferred, F = 96, 500 C/(mol e) is the Faraday constant, andQis the reaction quotient.At the common reference temperture of 298 K, substituting eachconstant into the equation the result isE = E°0.0592 Vnlog10Q ▼Was either rounded differently or used a different number of significant figureAlthough the reaction given in the introduction is at an elevated temperature, the standard cell potential at 25 °C is used inpotential under non-standard conditions.Part EWhat is the cell potential for the reactionE =at 57 °C when [Fe²+] == 2.90 M and [Mg2+] == 0.210 MExpress your answer to three significant figures and include the appropriate units.►View Available Hint(s)SubmitμÅValueProvide FeedbackUnitsMg(s) + Fe2+ (aq)→Mg2+ (aq) + Fe(s)?

Answered: Image /qna-images/answer/c9ffb854-7eda-404d-aab2-8f19d42dcbd1.jpg

Part E What is the cell potential for the reaction at 57 °C when [Fe2+] = 2.90 Mand [Mg2+] = 0.210 M. Express your answer to three significant figures and include the appropriate units. ►View Available Hint(s) E = μA Value Units Mg(s)+Fe2+ (aq)→Mg2+ (aq) + Fe(s) ?

Part E What is the cell potential for the reaction at 57 °C when [Fe2+] = 2.90 Mand [Mg2+] = 0.210 M. Express your answer to three significant figures and include the appropriate units. ►View Available Hint(s) E = μA Value Units Mg(s)+Fe2+ (aq)→Mg2+ (aq) + Fe(s) ?

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 5RQ: The Nernst equation allows determination of the cell potential for a galvanic cell at nonstandard...

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+ Introduction to the Nernst Equation
Learning Goal:
To learn how to use the Nernst equation.
The standard reduction potentials listed in any reference table are only
valid at the common reference temperature of 25 °C and standard
conditions of 1 M for solutions and 1 atm for gases. To calculate the
cell potential at nonstandard conditions, one uses the Nernst equation,
2.303 RT
E = E
nF
-log10 Q
where E is the potential in volts, E is the standard potential at 25 °C
in volts, R = 8.314 J/(K-mol) is the gas constant, T is the
temperature in kelvins, n is the number of moles of electrons
transferred, F = 96, 500 C/(mol e) is the Faraday constant, and
Qis the reaction quotient.
At the common reference temperture of 298 K, substituting each
constant into the equation the result is
E = E°
0.0592 V
n
log10
Q

▼
Was either rounded differently or used a different number of significant figure
Although the reaction given in the introduction is at an elevated temperature, the standard cell potential at 25 °C is used in
potential under non-standard conditions.
Part E
What is the cell potential for the reaction
E =
at 57 °C when [Fe²+] =
= 2.90 M and [Mg2+] =
= 0.210 M
Express your answer to three significant figures and include the appropriate units.
►View Available Hint(s)
Submit
μÅ
Value
Provide Feedback
Units
Mg(s) + Fe2+ (aq)→Mg2+ (aq) + Fe(s)
?

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