For the reaction2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 Vwhat is the cell potential at 25 ∘C∘C if the concentrations are [Co3+]=[Co3+]= 0.195 MM , [Co2+]=[Co2+]= 0.787 MM , and [Cl−]=[Cl−]= 0.341 MM , and the pressure of Cl2Cl2 is PCl2=PCl2= 5.30 atmatm ?Express your answer with the appropriate units. The Nernst equation is one of the most importantequations in electrochemistry. To calculate the cellpotential at non-standard-state conditions, the equation isE = E° –2.303 RT log10 Qwhere E is the potential in volts, E° is the standardpotential in volts, R is the gas constant, T is thetemperature in kelvins, n is the number of moles ofelectrons transferred, F is the Faraday constant, and Qis the reaction quotient. At standard temperature, 25 ° Cor 298 K, the equation has the formE = E° – (0.0592) log QThe reaction quotient has the usual form[products]"[reactants]"A table of standard reduction potentials gives the voltageat standard conditions, 1.00 M for all solutions and 1.00atm for all gases. The Nernst equation allows for thecalculation of the cell potential E at other conditions ofconcentration and pressure.

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Chemistry

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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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For the reaction

2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V

what is the cell potential at 25 ∘C∘C if the concentrations are [Co3+]=[Co3+]= 0.195 MM , [Co2+]=[Co2+]= 0.787 MM , and [Cl−]=[Cl−]= 0.341 MM , and the pressure of Cl2Cl2 is PCl2=PCl2= 5.30 atmatm ?

Express your answer with the appropriate units.

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° –
2.303 RT log10 Q
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. At standard temperature, 25 ° C
or 298 K, the equation has the form
E = E° – (0.0592) log Q
The reaction quotient has the usual form
[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.

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