Question

How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu2+ ions to produce 3.00 moles of copper metal?

Answer 1

3.22 hours

Answer 2

11580sec

Answer 3

1.61 hours

Answer 4

[AI-generated answer — Explain Bot]

To find the time required to produce 3.00 moles of copper metal, we need to use Faraday's Law of Electrolysis.

Faraday's Law states that the amount of substance (in moles) produced or consumed in an electrolysis process is directly proportional to the quantity of electric charge passed through the cell.

The formula is given by:
Moles of substance = (Electric charge passed) / (Faraday's constant)

To determine the electric charge passed, we use the formula:
Electric charge = Current (in amperes) × Time (in seconds)

The Faraday's constant is equal to the charge of one mole of electrons and is approximately 96,485 C/mol.

In this case, we have a constant current of 50.0 A and we want to produce 3.00 moles of copper.

Let's calculate the time required using the given information:

Moles of copper = 3.00 moles
Faraday's constant = 96,485 C/mol
Current = 50.0 A

First, we need to find the electric charge passed using the formula:
Electric charge = Current × Time

Rearranging the formula:
Time = Electric charge / Current

Substituting the values:
Time = (3.00 moles × 96,485 C/mol) / 50.0 A

Now, let's calculate the time required:
Time = (3.00 × 96485) / 50.0
Time = 57,891 / 50.0
Time = 1157.82 seconds

Therefore, it would take approximately 1157.82 seconds for a constant current of 50.0 A to produce 3.00 moles of copper metal in the electrolytic cell.