The Nernst equation is one of the most important equations inelectrochemistry. To calculate the cell potential at non-standard-stateconditions, the equation isE = E°log₁0 Qwhere E is the potential in volts, Eº is the standard potential in volts,R is the gas constant, T is the temperature in kelvins, ŉ is thenumber of moles of electrons transferred, F is the Faraday constant,and is the reaction quotient. Using the common referencetemperature, 25 °C or 298 K, the equation has the formE = E° -log Q2.303 RTnFQ:The reaction quotient has the usual form[products][reactants]-0.0592nA table of standard reduction potentials gives the voltage at standardconditions, 1.00 M for all solutions and 1.00 atm for all gases. TheNernst equation allows for the calculation of the cell potential E atother conditions of concentration and pressure.For the reaction2CO³+ (aq) + 2Cl(aq)→2Co²+ (aq) + Cl₂ (g). E° = 0.483 Vwhat is the cell potential at 25 °C if the concentrations are [Co³+] = 0.863 M, [Co²+] = 0.388 M, and [Cl¯] = 0.717 M, and the pressure of Cl₂ is PC1₂ = 2.80atm ?Express your answer with the appropriate units.► View Available Hint(s)E =SubmitμAValueProvide FeedbackUnitswww?Next

We will use the Nernst equation to calculate the Ecell

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. Using the common reference 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 Q= 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. For the reaction 2Co³+ (aq) + 2C1(aq) →2Co²+ (aq) + Cl₂(g). E = 0.483 V what is the cell potential at 25 °C if the concentrations are [Co³+] = 0.863 M. [Co²+] =0.388 M, and [Cl] = 0.717 M, and the pressure of Cl₂ is PC1₂ = 2.80 atm ? Express your answer with the appropriate units. ► View Available Hint(s) Submit LA Value Provide Feedback 3 → Units ? Next >

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. Using the common reference 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 Q= 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. For the reaction 2Co³+ (aq) + 2C1(aq) →2Co²+ (aq) + Cl₂(g). E = 0.483 V what is the cell potential at 25 °C if the concentrations are [Co³+] = 0.863 M. [Co²+] =0.388 M, and [Cl] = 0.717 M, and the pressure of Cl₂ is PC1₂ = 2.80 atm ? Express your answer with the appropriate units. ► View Available Hint(s) Submit LA Value Provide Feedback 3 → Units ? Next >

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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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…
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For the cell shown, the measured cell potential, Ecell, is −0.3627 V at 25 °C. Pt(s) | H2(g,0.735 atm) | H+(aq,? M) || Cd2+(aq,1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, ?o, are 2H+(aq)+2e−⟶H2(g) ?o=0.00 V Cd2+(aq)+2e−⟶Cd(s) ?o=−0.403 V Calculate the H+ concentration in M.
+ 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…