If a current of 0.850A is applied electrochemical cell above 60 min then what mass of Cu
To determine the mass of Cu that is deposited in the electrochemical cell, we need to use Faraday's law of electrolysis.
Faraday's law states that the amount of substance (in this case, Cu) deposited or liberated during electrolysis is directly proportional to the amount of charge (Q) passed through the cell. The proportionality constant is known as the Faraday constant (F).
The equation is given by:
m = (Q * M) / (n * F)
Where:
m = mass of substance deposited (in grams)
Q = charge passed through the cell (in coulombs)
M = atomic or molar mass of the substance (in grams per mole)
n = number of electrons involved in the reduction or oxidation reaction
F = Faraday constant (96500 C/mol)
First, let's calculate the charge passed through the cell in coulombs:
Q = I * t
Where:
I = current (in amperes)
t = time (in seconds)
Given:
I = 0.850 A
t = 60 min = 60 * 60 = 3600 seconds
Q = 0.850 A * 3600 s
Q = 3060 C
The atomic mass of Cu (M) is approximately 63.55 g/mol, and for the reduction of Cu2+ to Cu, two electrons (n = 2) are involved.
Now, let's substitute the values into the equation to find the mass (m):
m = (Q * M) / (n * F)
m = (3060 C * 63.55 g/mol) / (2 * 96500 C/mol)
m ≈ 1.61 g
Therefore, approximately 1.61 grams of Cu will be deposited in the electrochemical cell after 60 minutes if a current of 0.850A is applied.