Calculate the minimum time, in minutes, required to deposit 40g of copper using a current of 20A.

To calculate the minimum time required to deposit 40g of copper using a current of 20A, we need to use the Faraday's law of electrolysis.

Faraday's Law states that the amount of substance deposited or liberated during electrolysis is directly proportional to the quantity of electricity passed through the cell.

The formula to calculate the amount of substance deposited is:
Amount of Substance Deposited (in grams) = (Current (in Amperes) * Time (in seconds) * Atomic Mass) / (Faraday's Constant)

In this case, we want to find the minimum time required to deposit 40g of copper using a current of 20A.

First, we need to find the atomic mass of copper. The atomic mass of copper (Cu) is approximately 63.55 g/mol.

Next, we need to find Faraday's Constant, which is 96,485 Coulombs per mole.

Now we can rearrange the formula to solve for time.

Time (in seconds) = (Amount of Substance Deposited (in grams) * Faraday's Constant) / (Current (in Amperes) * Atomic Mass)

Substituting in the values:
Time (in seconds) = (40g * 96,485 C/mol) / (20A * 63.55 g/mol)

Now we can calculate the answer.

Time (in seconds) = (385,940 C) / (1,271 A)
Time (in seconds) ≈ 303.74 seconds

Since the question asks for the time in minutes, we can convert seconds to minutes by dividing the result by 60.

Time (in minutes) ≈ 303.74 seconds / 60
Time (in minutes) ≈ 5.06 minutes

Therefore, the minimum time required to deposit 40g of copper using a current of 20A is approximately 5.06 minutes.