How many grams of Ag(s) could be plated out on the cathode of an electrolytic cell...
How many grams of Ag(s) could be plated out on the cathode of an electrolytic cell by the passage of 5.0 Amps of current through AgNO3 solution for 1 hour?
| A. |
5.2 x 10-5 g |
|
| B. |
0.19 g |
|
| C. |
20 g |
|
| D. |
5.5 x 10-3 g |
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How many grams of Ag(s) could be plated out on the cathode of an
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An object of jewelry has a surface area of 4.20 cm2. It is to be plated with silver (Ag) to a depth of 30.0 eters, requiring a total of 0.0126 cm3 of Ag. Given the density of silver (10.5 g/cm2), how long will it take to electroplate the silver using an electrolytic cell with the object connected to the cathode, a solution of AgNO3 (aq) and a current of 2.48 mA? Assume 100% cell efficiency.
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3. How many grams of Ag(s) could be plated out on the cathode of an electrolytic cell by the passage of 5.0 Amps of current through AgNO3 solution for 1 hour? Faraday's number = 96485 Coul/mol. a) 5.5 x 10-ºg b) 0.19 g c) 5.2 x 105 g d) 2.0 g e) 20 g
What mass of silver is deposited on the cathode of an electrolytic cell if an electric current of 2.86 A is run through a solution of AgNO3 for one hour? Select one: O a. 11.5 g O b. 5.76 g O c. Og O d. 0.11 g o e. 0.192 g
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An object of jewelry has a surface area of 4.20 cm2. It is to be plated with silver (Ag) to a depth of 30.0 eters, requiring a total of 0.0126 cm3 of Ag. Given the density of silver (10.5 g/cm2), how long will it take to electroplate the silver using an electrolytic cell with the object connected to the cathode, a solution of AgNO3 (aq) and a current of 2.48 mA? Assume 100% cell efficiency.
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