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A. What is the cell notation of the set-up? B. What is the standard cell potential (Eºcell)? C. If the measured cell potential (Ecell) is 1.800V, what is the concentration of Au³*? After determining the gold ion concentration, Tanjiro then proceeded with the electrolysis process. He electroplated the katana using 250.0 mL of the gold solution with a current of 3.20A. D. How long (in hrs) will it take to electroplate the katana assuming that all gold ions are converted to solid gold? E. What is the mass of the electroplated gold?

A. What is the cell notation of the set-up? B. What is the standard cell potential (Eºcell)? C. If the measured cell potential (Ecell) is 1.800V, what is the concentration of Au³*? After determining the gold ion concentration, Tanjiro then proceeded with the electrolysis process. He electroplated the katana using 250.0 mL of the gold solution with a current of 3.20A. D. How long (in hrs) will it take to electroplate the katana assuming that all gold ions are converted to solid gold? E. What is the mass of the electroplated gold?

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A. What is the cell notation of the set-up? B. What is the standard cell potential (Eºcell)? C. If the measured cell potential (Ecell) is 1.800V, what is the concentration of Au³+? After determining the gold ion concentration, Tanjiro then proceeded with the electrolysis process. He electroplated the katana using 250.0 mL of the gold solution with a current of 3.20A. D. How long (in hrs) will it take to electroplate the katana assuming that all gold ions are converted to solid gold? E. What is the mass of the electroplated gold?
Transcribed Image Text:A. What is the cell notation of the set-up? B. What is the standard cell potential (Eºcell)? C. If the measured cell potential (Ecell) is 1.800V, what is the concentration of Au³+? After determining the gold ion concentration, Tanjiro then proceeded with the electrolysis process. He electroplated the katana using 250.0 mL of the gold solution with a current of 3.20A. D. How long (in hrs) will it take to electroplate the katana assuming that all gold ions are converted to solid gold? E. What is the mass of the electroplated gold?
3. Tanjiro, a Chem 17.1 student, found a prehistoric katana during his trip to Japan. He inspected the katana and realized that it was made out of gold. Upon closer inspection, Tanjiro noticed that it had a lot of chips and scratches, signifying that it had been used in battle long ago. Wanting to restore the katana to its original state, Tanjiro used his knowledge in Chem 17.1 to electroplate gold into the surface of the katana using an ore his father found on their backyard. Tanjiro proceeded with the electroplating process, however, he realized that the concentration of the gold ions present in the solution is unknown, making the electroplating process difficult to plan. He then decided to use a galvanic cell to obtain the gold ion concentration. He used the half-cell reactions below: Au³+ (aq) + 3e → Au(s) E° = +1.520V E° = -0.230V Ni²+ (aq) + 2e → Ni(s) Given: [Ni²+] = 0.050 M FMNI = 58.69 g/mol FMAU = 196.97 g/mol
Transcribed Image Text:3. Tanjiro, a Chem 17.1 student, found a prehistoric katana during his trip to Japan. He inspected the katana and realized that it was made out of gold. Upon closer inspection, Tanjiro noticed that it had a lot of chips and scratches, signifying that it had been used in battle long ago. Wanting to restore the katana to its original state, Tanjiro used his knowledge in Chem 17.1 to electroplate gold into the surface of the katana using an ore his father found on their backyard. Tanjiro proceeded with the electroplating process, however, he realized that the concentration of the gold ions present in the solution is unknown, making the electroplating process difficult to plan. He then decided to use a galvanic cell to obtain the gold ion concentration. He used the half-cell reactions below: Au³+ (aq) + 3e → Au(s) E° = +1.520V E° = -0.230V Ni²+ (aq) + 2e → Ni(s) Given: [Ni²+] = 0.050 M FMNI = 58.69 g/mol FMAU = 196.97 g/mol
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