Question

Which of the following is true for the amount of copper deposited during electrolysis? Molar mass of Cu =63.5 g/mol F = 96485C/mol

Select the correct response:

1• Cu(1)CI 5.00 A, 10 min Mass of Cu deposited =4.97g

2• Cu(II)C12 2.00 A 30 min Mass of Cu deposited = 1.185 g

3• Cu(1)CI 2.00A 30 min Mass of Cu deposited = 0.5925 g

4• Cu(II)C12 5.00 A, 10 min Mass of Cu deposited =2.485g

Answer 1

The correct response is:

1• Cu(1)CI 5.00 A, 10 min Mass of Cu deposited =4.97g

This is true because by using Faraday's laws of electrolysis, the mass of copper deposited is directly proportional to the current and time.

The molar mass of copper is 63.5 g/mol, and the Faraday constant is 96485 C/mol.

Cu(1)CI has a current of 5.00 A and a time of 10 min, so the mass of Cu deposited can be calculated as:

mass of Cu deposited = (5.00A * 10min * 96485C/mol) / (63.5g/mol) = 4.97g

The other options are not true as they don't match the given current and time.