Question
If a current of 4.00x10^-3 A is maintained for 10s in this electrochemical cell then the mass of ethanol would be
Answers
GPT 3.5
To calculate the mass of ethanol produced, we need to use Faraday's law of electrolysis.
Faraday's law states that the amount of substance produced or consumed during an electrochemical reaction is directly proportional to the quantity of charge passing through the cell.
The equation for Faraday's law is:
Mass (g) = (Current (A) x Time (s) x Molar mass (g/mol)) / (Faraday constant (C/mol))
Given:
Current = 4.00x10^-3 A
Time = 10 s
Molar mass of ethanol = 46.07 g/mol (rounded to two decimal places, can be verified from the periodic table)
Faraday constant = 96,485 C/mol
Now, let's calculate the mass of ethanol produced:
Mass = (4.00x10^-3 A x 10 s x 46.07 g/mol) / 96,485 C/mol
Mass = (4.00x10^-2 C x 46.07 g/mol) / 96,485 C/mol
Mass = 0.04603 g
Therefore, the mass of ethanol produced in this electrochemical cell would be approximately 0.046 g.
Faraday's law states that the amount of substance produced or consumed during an electrochemical reaction is directly proportional to the quantity of charge passing through the cell.
The equation for Faraday's law is:
Mass (g) = (Current (A) x Time (s) x Molar mass (g/mol)) / (Faraday constant (C/mol))
Given:
Current = 4.00x10^-3 A
Time = 10 s
Molar mass of ethanol = 46.07 g/mol (rounded to two decimal places, can be verified from the periodic table)
Faraday constant = 96,485 C/mol
Now, let's calculate the mass of ethanol produced:
Mass = (4.00x10^-3 A x 10 s x 46.07 g/mol) / 96,485 C/mol
Mass = (4.00x10^-2 C x 46.07 g/mol) / 96,485 C/mol
Mass = 0.04603 g
Therefore, the mass of ethanol produced in this electrochemical cell would be approximately 0.046 g.