Silver can be electroplated at the cathode of an electrolysis ...

Question

Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag⁺(aq) + e^– → Ag(s) What mass of silver would plate onto the cathode if a current of 6.8 A flowed through the cell for 72 min?

Accepted Answer

First, we need to understand the relationship between current, time, and the amount of substance produced in an electrolysis reaction. This is given by Faraday's laws of electrolysis. According to the first law, the mass of a substance produced at an electrode during electrolysis is directly proportional to the quantity of electricity that passes through the electrolyte. The quantity of electricity can be calculated by multiplying the current (in amperes) by the time (in seconds).. Next, we need to convert the time given in minutes to seconds because the SI unit of time in this context is the second. This can be done by multiplying the time in minutes by 60.. Then, we calculate the total charge passed through the cell by multiplying the current by the time in seconds. This gives us the total charge in coulombs.. Next, we need to calculate the number of moles of electrons transferred. This can be done by dividing the total charge by the charge of one mole of electrons, which is known as Faraday's constant (approximately 96485 C/mol).. Finally, we can calculate the mass of silver plated out. From the half-reaction, we can see that one mole of silver ions (Ag+) reacts with one mole of electrons to form one mole of silver atoms (Ag). Therefore, the number of moles of silver plated out is equal to the number of moles of electrons transferred. The mass can then be calculated by multiplying the number of moles by the molar mass of silver (approximately 107.87 g/mol).

Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag⁺(aq) + e^– → Ag(s) What mass of silver would plate onto the cathode if a current of 6.8 A flowed through the cell for 72 min?

비슷한 문제에 대한 검증된 영상 답변:

주요 개념

Electrolysis

Faraday's Laws of Electrolysis

Current and Charge

Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag+(aq) + e– → Ag(s) What mass of silver would plate onto the cathode if a current of 6.8 A flowed through the cell for 72 min?

비슷한 문제에 대한 검증된 영상 답변:

주요 개념

Electrolysis

Faraday's Laws of Electrolysis

Current and Charge

Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag⁺(aq) + e^– → Ag(s) What mass of silver would plate onto the cathode if a current of 6.8 A flowed through the cell for 72 min?