5a. Calculating the Concentration of Ag+ In the cell: Ref|| Ag|Ag(s) The left half-cell is a reference electrode (Ref) with a potential of 0.27 V. The right half-cell is based on the process: Age Ag(s) E0 = 0.80 V The electromotive force (EMF) of the cell is E = 0.31 V. The concentration of Ag+ in the right half-cell can be calculated using the Nernst equation: E = E⁰ 0.0592 log red] 5b. Determining the Equilibrium Constant B₂ In another cell with the same reference electrode: Ref|| Ag (1.00 x 10-¹ M)|Ag(s) The right half-cell has a volume of 400 mL. To this, 100 mL of a 0.100 M solution of Na2S2O3 is added, leading to the following equilibrium: Ag+ + 2S20 [Ag(S2O3)2]3 ẞ2 After this addition, the EMF of the cell is E = -0.20 V. The right half-cell potential and the concentrations of Ag+, S₂O¾¾¯, and [Ag(S2O3)2]³ in the right half-cell can be calculated. Using these concentrations, ẞ2 can be determined. 5c. Calculating the Standard Electrode Potential To calculate the standard electrode potential E for the reduction of [Ag(S2O3)2]³- to Ag(s) and S20, the following process is used: [Ag(S2O3)2]+e → Ag(s) + 2S20 E⁰
5a. Calculating the Concentration of Ag+ In the cell: Ref|| Ag|Ag(s) The left half-cell is a reference electrode (Ref) with a potential of 0.27 V. The right half-cell is based on the process: Age Ag(s) E0 = 0.80 V The electromotive force (EMF) of the cell is E = 0.31 V. The concentration of Ag+ in the right half-cell can be calculated using the Nernst equation: E = E⁰ 0.0592 log red] 5b. Determining the Equilibrium Constant B₂ In another cell with the same reference electrode: Ref|| Ag (1.00 x 10-¹ M)|Ag(s) The right half-cell has a volume of 400 mL. To this, 100 mL of a 0.100 M solution of Na2S2O3 is added, leading to the following equilibrium: Ag+ + 2S20 [Ag(S2O3)2]3 ẞ2 After this addition, the EMF of the cell is E = -0.20 V. The right half-cell potential and the concentrations of Ag+, S₂O¾¾¯, and [Ag(S2O3)2]³ in the right half-cell can be calculated. Using these concentrations, ẞ2 can be determined. 5c. Calculating the Standard Electrode Potential To calculate the standard electrode potential E for the reduction of [Ag(S2O3)2]³- to Ag(s) and S20, the following process is used: [Ag(S2O3)2]+e → Ag(s) + 2S20 E⁰
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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![5a. Calculating the Concentration of Ag+
In the cell:
Ref|| Ag|Ag(s)
The left half-cell is a reference electrode (Ref) with a potential of 0.27 V.
The right half-cell is based on the process:
Age Ag(s) E0 = 0.80 V
The electromotive force (EMF) of the cell is E = 0.31 V. The concentration of Ag+ in the
right half-cell can be calculated using the Nernst equation:
E = E⁰
0.0592 log
red]
5b. Determining the Equilibrium Constant B₂
In another cell with the same reference electrode:
Ref|| Ag (1.00 x 10-¹ M)|Ag(s)
The right half-cell has a volume of 400 mL. To this, 100 mL of a 0.100 M solution of
Na2S2O3 is added, leading to the following equilibrium:
Ag+ + 2S20
[Ag(S2O3)2]3 ẞ2
After this addition, the EMF of the cell is E = -0.20 V. The right half-cell potential and the
concentrations of Ag+, S₂O¾¾¯, and [Ag(S2O3)2]³ in the right half-cell can be calculated.
Using these concentrations, ẞ2 can be determined.
5c. Calculating the Standard Electrode Potential
To calculate the standard electrode potential E for the reduction of [Ag(S2O3)2]³- to
Ag(s) and S20, the following process is used:
[Ag(S2O3)2]+e
→ Ag(s) + 2S20
E⁰](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff3af72d4-6516-4f0e-adeb-8608b46e21be%2F0ece25e8-89eb-42ef-aa08-1bf55c50dfd3%2Fa1081o_processed.png&w=3840&q=75)
Transcribed Image Text:5a. Calculating the Concentration of Ag+
In the cell:
Ref|| Ag|Ag(s)
The left half-cell is a reference electrode (Ref) with a potential of 0.27 V.
The right half-cell is based on the process:
Age Ag(s) E0 = 0.80 V
The electromotive force (EMF) of the cell is E = 0.31 V. The concentration of Ag+ in the
right half-cell can be calculated using the Nernst equation:
E = E⁰
0.0592 log
red]
5b. Determining the Equilibrium Constant B₂
In another cell with the same reference electrode:
Ref|| Ag (1.00 x 10-¹ M)|Ag(s)
The right half-cell has a volume of 400 mL. To this, 100 mL of a 0.100 M solution of
Na2S2O3 is added, leading to the following equilibrium:
Ag+ + 2S20
[Ag(S2O3)2]3 ẞ2
After this addition, the EMF of the cell is E = -0.20 V. The right half-cell potential and the
concentrations of Ag+, S₂O¾¾¯, and [Ag(S2O3)2]³ in the right half-cell can be calculated.
Using these concentrations, ẞ2 can be determined.
5c. Calculating the Standard Electrode Potential
To calculate the standard electrode potential E for the reduction of [Ag(S2O3)2]³- to
Ag(s) and S20, the following process is used:
[Ag(S2O3)2]+e
→ Ag(s) + 2S20
E⁰
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