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Part A For the reaction what is the cell potential at 25°C if the concentrations are [Co³+] = 0.858 M, [Co²+] = 0.159 M, and [CI-] = 0.744 M, and the pressure of Cl2 is Pc₂ = 7.10 atm ? Express your answer with the appropriate units. ► View Available Hint(s) F O M HÅ 2Co³+ (aq) + 2Cl(aq)-2Co²+ (aq) + Cl₂ (g). E = 0.483 V 3+ Value Units ?

Part A For the reaction what is the cell potential at 25°C if the concentrations are [Co³+] = 0.858 M, [Co²+] = 0.159 M, and [CI-] = 0.744 M, and the pressure of Cl2 is Pc₂ = 7.10 atm ? Express your answer with the appropriate units. ► View Available Hint(s) F O M HÅ 2Co³+ (aq) + 2Cl(aq)-2Co²+ (aq) + Cl₂ (g). E = 0.483 V 3+ Value Units ?

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.144QP
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he Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non- tandard-state conditions, the equation is E = E- 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, n is the number of moles of electrons transferred, F is the Faraday constant, and is the reaction quotient. Part A For the reaction 2Co³+ (aq) + 2Cl(aq)→2Co²+ (aq) + Cl₂ (g). E = 0.483 V what is the cell potential at 25°C if the concentrations are [Co³+] = 0.858 M, [Co2+] = 0.159 M, and [Cl] = 0.744 M, and the pressure of Cl2 is Pc₂ = 7.10 atm ? Express your answer with the appropriate units. ►View Available Hint(s) E = Submit D μA 2.303 RT n.F Value Units ?
Transcribed Image Text:he Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non- tandard-state conditions, the equation is E = E- 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, n is the number of moles of electrons transferred, F is the Faraday constant, and is the reaction quotient. Part A For the reaction 2Co³+ (aq) + 2Cl(aq)→2Co²+ (aq) + Cl₂ (g). E = 0.483 V what is the cell potential at 25°C if the concentrations are [Co³+] = 0.858 M, [Co2+] = 0.159 M, and [Cl] = 0.744 M, and the pressure of Cl2 is Pc₂ = 7.10 atm ? Express your answer with the appropriate units. ►View Available Hint(s) E = Submit D μA 2.303 RT n.F Value Units ?
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