Question
Calculate the mass of copper that could be produced in an electrolytic cell when a current of
6.5 A is applied for 41.5 min
6.5 A is applied for 41.5 min
Answers
GPT 3.5
To calculate the mass of copper that could be produced in an electrolytic cell, we need to use Faraday's law of electrolysis.
The equation is:
Mass of substance = (Current × Time) / (Faraday's constant × number of moles of electrons per mole of copper)
First, let's calculate the number of moles of electrons per mole of copper. Since copper has a +2 charge, it requires 2 moles of electrons to produce 1 mole of copper.
Number of moles of electrons per mole of copper = 2
Next, let's calculate the mass of copper using the formula mentioned above:
Mass of copper = (6.5 A × 41.5 min) / (Faraday's constant × 2)
The Faraday's constant is approximately 96,500 C/mol.
Mass of copper = (6.5 A × 41.5 min) / (96,500 C/mol × 2)
Now we can calculate the mass of copper:
Mass of copper = (6.5 A × 41.5 min) / (96,500 C/mol × 2)
≈ 136.14 g
Therefore, the mass of copper that could be produced in an electrolytic cell when a current of 6.5 A is applied for 41.5 min is approximately 136.14 grams.
The equation is:
Mass of substance = (Current × Time) / (Faraday's constant × number of moles of electrons per mole of copper)
First, let's calculate the number of moles of electrons per mole of copper. Since copper has a +2 charge, it requires 2 moles of electrons to produce 1 mole of copper.
Number of moles of electrons per mole of copper = 2
Next, let's calculate the mass of copper using the formula mentioned above:
Mass of copper = (6.5 A × 41.5 min) / (Faraday's constant × 2)
The Faraday's constant is approximately 96,500 C/mol.
Mass of copper = (6.5 A × 41.5 min) / (96,500 C/mol × 2)
Now we can calculate the mass of copper:
Mass of copper = (6.5 A × 41.5 min) / (96,500 C/mol × 2)
≈ 136.14 g
Therefore, the mass of copper that could be produced in an electrolytic cell when a current of 6.5 A is applied for 41.5 min is approximately 136.14 grams.