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
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.