If 1.70 liters of 0.670 M CuSO4 solution is electrolyzed by passing 4.70 amps through the solution for 3.00 hr using inert electrodes.
To find the amount of copper (Cu) deposited during the electrolysis process, you need to use Faraday's law of electrolysis.
Faraday's law states that the amount of substance (in this case, copper) produced or consumed during electrolysis is directly proportional to the amount of electricity passed through the solution. The equation for Faraday's law is:
n = (Q) / (F * z)
Where:
n is the number of moles of substance produced or consumed
Q is the total charge passed through the solution (in coulombs)
F is the Faraday constant (96,485 C/mol)
z is the number of moles of electrons transferred per mole of substance
In this case, we want to find the number of moles of copper produced (n).
First, we need to calculate the total charge passed through the solution (Q).
Q = I * t
Where:
I is the current (4.70 amps)
t is the time (3.00 hours)
Next, we substitute the values into the equation to find the total charge passed through the solution:
Q = (4.70 A) * (3.00 hr)
Now, we need to convert the time from hours to seconds:
t_sec = t * 60 * 60
t_sec = 3.00 hr * 60 min/hr * 60 sec/min
Finally, we can substitute the values into the equation for Q:
Q = (4.70 A) * (3.00 hr * 60 min/hr * 60 sec/min)
Once you have the value for Q, you can substitute it into Faraday's law equation to find the number of moles of copper produced (n). Then, you can convert the moles of copper to grams by using the molar mass of copper (63.55 g/mol).