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▼ 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+] = 0.425 M. [Co²+] = 0.384 M, and [Cl] = 0.337 M, and the pressure of Cl₂ is PC₁₂ = 8.30 atm ? Express your answer with the appropriate units. ► View Available Hint(s) E= HA Value Units S ?

▼ 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+] = 0.425 M. [Co²+] = 0.384 M, and [Cl] = 0.337 M, and the pressure of Cl₂ is PC₁₂ = 8.30 atm ? Express your answer with the appropriate units. ► View Available Hint(s) E= HA Value Units S ?

Chemistry
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° - 2.303 RT nF -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] 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 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+] = 0.425 M, [Co²+] = 0.384 M, and [Cl] = 0.337 M, and the pressure of Cl₂ is Pc₂ = 8.30 atm ? Express your answer with the appropriate units. ► View Available Hint(s) E= Submit μA Value Provide Feedback Units ? Next >
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 nF -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] 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 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+] = 0.425 M, [Co²+] = 0.384 M, and [Cl] = 0.337 M, and the pressure of Cl₂ is Pc₂ = 8.30 atm ? Express your answer with the appropriate units. ► View Available Hint(s) E= Submit μA Value Provide Feedback Units ? Next >
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