Homework Help is Here – Start Your Trial Now!
Science
Chemistry
The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard - state conditions, the equation is EE-2.303RTn Flog10Q where E is the potential in volts, E is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q is the reaction quotient. Using the common reference temperature, 25 °C or 298 K, the equation has the form E E-(0.0592n)logQ The reaction quotient has the usual form Q = [products]x[ reactants]y A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure. Part A For the reaction 2Co3+ (aq) + 2CI-(aq)-> 2Co2 + (aq )+C12(g). E 0.483 V what is the cell potential at 25°

The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard - state conditions, the equation is EE-2.303RTn Flog10Q where E is the potential in volts, E is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q is the reaction quotient. Using the common reference temperature, 25 °C or 298 K, the equation has the form E E-(0.0592n)logQ The reaction quotient has the usual form Q = [products]x[ reactants]y A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure. Part A For the reaction 2Co3+ (aq) + 2CI-(aq)-> 2Co2 + (aq )+C12(g). E 0.483 V what is the cell potential at 25°

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
The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is E = E-2.303RTn Flog 10Q where E is the potential in volts, Eo is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q is the reaction quotient. Using the common reference temperature, 25 °C or 298 K, the equation has the form E = E-(0.0592n)logQ The reaction quotient has the usual form Q = [products]x[ reactants]y A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure. Part A For the reaction 2C03 + (aq) + 2CI-(aq)-> 2Co2 + (aq )+ Cl2(g). E = 0.483 V what is the cell potential at 25° C if the concentrations are [Co3+] = 9.20\times 10-2 M, [Co2+] 0.758 M, and [CI-] = 0.895 M, and the pressure of C12 is PC12 = 3.10 atm ?
Transcribed Image Text:The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is E = E-2.303RTn Flog 10Q where E is the potential in volts, Eo is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q is the reaction quotient. Using the common reference temperature, 25 °C or 298 K, the equation has the form E = E-(0.0592n)logQ The reaction quotient has the usual form Q = [products]x[ reactants]y A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure. Part A For the reaction 2C03 + (aq) + 2CI-(aq)-> 2Co2 + (aq )+ Cl2(g). E = 0.483 V what is the cell potential at 25° C if the concentrations are [Co3+] = 9.20\times 10-2 M, [Co2+] 0.758 M, and [CI-] = 0.895 M, and the pressure of C12 is PC12 = 3.10 atm ?
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Potentiometric Titrations
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.
Similar questions
  • SEE MORE QUESTIONS
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