+ The Nernst EquationThe Nernst equation is one of the most important equations in electrochemistry.To calculate the cell potential at non-standard-state conditions, the equation iE=E2.303 RT log10 Qwhere E is the potential in volts, Eo is the standard potential in volts, R is thegas constant, T is the temperature in kelvins, 12 is the number of moles ofelectrons transferred, Fis the Faraday constant, and is the reactionquotient. Using the common reference temperature, 25 °C or 298 K, theequation has the formE = ED (0.0592) log QThe reaction quotient has the usual formQ[products[reactantsA table of standard reduction potentials gives the voltage at standardconditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernstequation allows for the calculation of the cell potential E at other conditions ofconcentration and pressure.Part AFor the reaction2Co²+ (aq) + 2Cl(aq) +2Co²+ (aq) + Ch₂(g). E0.483 Vwhat is the cell potential at 25°C if the concentrations are [Co¹+1=0.261 M. [Co²+] = 0.269 M, and [C1-1=0.694 M, and the pressure of Cl₂ is PC₁₂ = 7.50 atm ?Express your answer with the appropriate units.▸ View Available Hint(s)E=MμAValueSubmit Previous AnswersProvide FeedbackUnits?* Incorrect; Try Again; 5 attempts remaining33 aReview | Constants | Period

We will use the Nernst equation to calculate the Ecell E=Eo-RTnFlnQat 25ocE=E0-0.0592nlogQ the given…

For the reaction 2Co (aq) + 2Cl(aq) +2Co²+ (aq) + Cl₂(g). E=0.483 V what is the cell potential at 25°C if the concentrations are [Co³|=0.261 M. [Co²+1 0.269 M. and [C]]=0.694 M, and the pressure of Cl₂ is Pci, -7.50 atm? Express your answer with the appropriate units. ▸ View Available Hint(s) E= Value Submit Previous Answers Units ? * Incorrect; Try Again; 5 attempts remaining

For the reaction 2Co (aq) + 2Cl(aq) +2Co²+ (aq) + Cl₂(g). E=0.483 V what is the cell potential at 25°C if the concentrations are [Co³|=0.261 M. [Co²+1 0.269 M. and [C]]=0.694 M, and the pressure of Cl₂ is Pci, -7.50 atm? Express your answer with the appropriate units. ▸ View Available Hint(s) E= Value Submit Previous Answers Units ? * Incorrect; Try Again; 5 attempts remaining

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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Question

+ The Nernst Equation
The Nernst equation is one of the most important equations in electrochemistry.
To calculate the cell potential at non-standard-state conditions, the equation i
E=E
2.303 RT log10 Q
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, 12 is the number of moles of
electrons transferred, Fis the Faraday constant, and is the reaction
quotient. Using the common reference temperature, 25 °C or 298 K, the
equation has the form
E = ED (0.0592) log Q
The reaction quotient has the usual form
Q
[products
[reactants
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
2Co²+ (aq) + 2Cl(aq) +2Co²+ (aq) + Ch₂(g). E
0.483 V
what is the cell potential at 25°C if the concentrations are [Co¹+1=0.261 M. [Co²+] = 0.269 M, and [C1-1=0.694 M, and the pressure of Cl₂ is PC₁₂ = 7.50 atm ?
Express your answer with the appropriate units.
▸ View Available Hint(s)
E=
M
μA
Value
Submit Previous Answers
Provide Feedback
Units
?
* Incorrect; Try Again; 5 attempts remaining
33 a
Review | Constants | Period

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