Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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
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...
See similar textbooks
icon
Related questions
Question
100%
Thank you!
+ 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
Transcribed Image Text:+ 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) ?
Transcribed Image Text:▼ 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) ?
Expert Solution
steps

Step by step

Solved in 2 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Electroanalytical Techniques
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS