Using a current of 4.75A how many minutes does it takes to plate onto a sculpture 1.50g of CuSO4 solution?
You can't plate CuSO4. You can plat Cu metal.
How a current of 4.75A, how many minutes does it takes to plate onto a sculpture 1.50g of CuSO4 solution?
wtf ms. sue but I will if you want me to?
To determine the time required to plate 1.50g of CuSO4 solution onto a sculpture using a current of 4.75A, you'll need to use 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 electric charge passed through the electrolyte. The formula for Faraday's law is:
\(Q = I \times t\),
where:
Q = amount of charge (Coulombs)
I = current (Amperes)
t = time (seconds)
First, let's convert the current to Coulombs per second (C/s) by multiplying it by the amount of time in seconds.
Given that 1 Ampere (A) is equal to 1 Coulomb per second (C/s), we can write:
\(4.75A \times t\) = Q
Next, we need to convert the mass of the CuSO4 solution to moles. The molar mass of CuSO4 is:
Cu = 63.55 g/mol
S = 32.06 g/mol
O = 16.00 g/mol (4 oxygen atoms)
Total molar mass = 63.55 + 32.06 + (16.00 * 4) = 159.61 g/mol
Using the formula:
\(moles = mass / molar mass\),
we can find the number of moles of CuSO4:
\(moles = 1.50g / 159.61 g/mol\).
Finally, we can use Faraday's law to find the time required:
\(4.75A \times t = (moles \times Faraday's constant)\),
where Faraday's constant is 96,485 Coulombs per mole.
Rearranging the equation to solve for time (t):
\(t = (moles \times Faraday's constant) / 4.75A\).
Substituting the values:
\(t = (moles \times 96,485 C/mol) / 4.75A\).
Calculate the value of moles, then substitute it in the equation above to find the time (t) in seconds. To convert from seconds to minutes, divide the value by 60.
So, to determine the time required to plate 1.50g of CuSO4 solution onto the sculpture using a current of 4.75A, follow the steps above.