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surrounded by a 0.834 mol/L solution of ZnCl₂. The second half cell is a standard hydrogen electrode (SHE), which consists of an inert platinum electrode in contact with an aqueous solution with pH-0 and hydrogen gas (H₂) at a partial pressure of 1 bar. The temperature is 25 °C and all solutions and gases can be considered ideal.. Part a) Specify the cathode and anode in the electrochemical cell, the corresponding half reactions and the overall redox reaction. Part b) Calculate the difference between the standard reduction potentials, AE, of the cathode and the anode for this electrochemical cell and the standard reaction free energy A, G of the underlying redox reaction. Part c) Provide a mathematical expression for the reaction coefficient of the redox reaction in this electrochemical cell.

surrounded by a 0.834 mol/L solution of ZnCl₂. The second half cell is a standard hydrogen electrode (SHE), which consists of an inert platinum electrode in contact with an aqueous solution with pH-0 and hydrogen gas (H₂) at a partial pressure of 1 bar. The temperature is 25 °C and all solutions and gases can be considered ideal.. Part a) Specify the cathode and anode in the electrochemical cell, the corresponding half reactions and the overall redox reaction. Part b) Calculate the difference between the standard reduction potentials, AE, of the cathode and the anode for this electrochemical cell and the standard reaction free energy A, G of the underlying redox reaction. Part c) Provide a mathematical expression for the reaction coefficient of the redox reaction in this electrochemical cell.

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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uncements US es lock ASUO S ourse Policies rces sibility AZ 35 ments nline Tutoring We are building an electrochemical cell. The first half cell consists of a zinc electrode surrounded by a 0.834 mol/L solution of ZnCl₂. The second half cell is a standard hydrogen electrode (SHE), which consists of an inert platinum electrode in contact with an aqueous solution with pH-0 and hydrogen gas (H₂) at a partial pressure of 1 bar. The temperature is 25 °C and all solutions and gases can be considered ideal. Part a) Specify the cathode and anode in the electrochemical cell, the corresponding half reactions and the overall redox reaction. Part b) Calculate the difference between the standard reduction potentials, AE, of the cathode and the anode for this electrochemical cell and the standard reaction free energy A, G of the underlying redox reaction. Part c) Provide a mathematical expression for the reaction coefficient of the redox reaction in this electrochemical cell. Part d) Calculate the electromotive force AD and the thermodynamic driving force AG for the electrochemical cell under the current conditions. Parte) Sodium hydroxide (NaOH) is added to the solution in the hydrogen electrode until the pH of the solution is equal to 7. Recalculate the electromotive force AD and the thermodynamic driving force AG for the electrochemical cell under these conditions. Part f) What would happen if instead of NaOH, we added, ammonium chloride (NII CI) to the solution in the standard hydrogen electrode (pH=0) until the NII, Cl concentration reaches 0,200 mol/L. Determine the electromotive force and the thermodynamic driving force AC for the electrochemical cell under these conditions The A of the ammonium ion is 9.25. (Think first before you start any
Transcribed Image Text:uncements US es lock ASUO S ourse Policies rces sibility AZ 35 ments nline Tutoring We are building an electrochemical cell. The first half cell consists of a zinc electrode surrounded by a 0.834 mol/L solution of ZnCl₂. The second half cell is a standard hydrogen electrode (SHE), which consists of an inert platinum electrode in contact with an aqueous solution with pH-0 and hydrogen gas (H₂) at a partial pressure of 1 bar. The temperature is 25 °C and all solutions and gases can be considered ideal. Part a) Specify the cathode and anode in the electrochemical cell, the corresponding half reactions and the overall redox reaction. Part b) Calculate the difference between the standard reduction potentials, AE, of the cathode and the anode for this electrochemical cell and the standard reaction free energy A, G of the underlying redox reaction. Part c) Provide a mathematical expression for the reaction coefficient of the redox reaction in this electrochemical cell. Part d) Calculate the electromotive force AD and the thermodynamic driving force AG for the electrochemical cell under the current conditions. Parte) Sodium hydroxide (NaOH) is added to the solution in the hydrogen electrode until the pH of the solution is equal to 7. Recalculate the electromotive force AD and the thermodynamic driving force AG for the electrochemical cell under these conditions. Part f) What would happen if instead of NaOH, we added, ammonium chloride (NII CI) to the solution in the standard hydrogen electrode (pH=0) until the NII, Cl concentration reaches 0,200 mol/L. Determine the electromotive force and the thermodynamic driving force AC for the electrochemical cell under these conditions The A of the ammonium ion is 9.25. (Think first before you start any
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Electrochemical cell considered has two electrodes:

  • Zn rod in 0.834 mol/L Zinc chloride solution 
  • Standard Hydrogen Electrode (SHE), pH = 0

Temperature is 25 oC 

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