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.
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.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.9: Corrosion: Redox Reactions In The Environment
Problem 2.5ACP: Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in...
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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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb0341e13-6796-4d12-951d-e871d1397669%2Fe5b86630-8a1b-439c-a617-cba17f7e142a%2Fcotg3dj.png&w=3840&q=75)
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° –
2.303 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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