calculate the mass of copper deposited when a current of 0.5
amphere was passed through a solution of copper (ii) chloride for 45 minutes in an electrolytic cell (eu=63.IF=96500C)
Coulombs = amperes x seconds
C = 0.5 x 45 x (60 sec/min) = 1350
96,500 coulombs will deposit 63.54/2 = 31.77 g Cu
63.54 g x (1350/96,500) = ? g Cu deposited.
0.89
To calculate the mass of copper deposited, you will need to use the formula:
Mass of copper = (Current × Time × Atomic mass of copper) / (Faraday's constant)
Let's plug in the given values into the formula:
Current = 0.5 A
Time = 45 minutes = 45 × 60 seconds = 2700 seconds
Atomic mass of copper = 63 g/mol
Faraday's constant (F) = 96500 C/mol
Now, calculate the mass of copper deposited.
Mass of copper = (0.5 A × 2700 s × 63 g/mol) / 96500 C
Mass of copper = (337.5 g·s/mol) / 96500 C
Mass of copper ≈ 0.0035 g
Therefore, approximately 0.0035 grams of copper will be deposited when a current of 0.5 A is passed through a solution of copper (II) chloride for 45 minutes in an electrolytic cell.
To calculate the mass of copper deposited, we need to use the equation that relates the amount of substance (in moles) to the mass and the molar mass of the substance.
First, let's determine the charge passed through the cell using Faraday's Law of Electrolysis:
Q = I * t
Where:
Q is the charge in coulombs (C)
I is the current in amperes (A)
t is the time in seconds (s)
Since the time given is in minutes, we need to convert it to seconds:
45 minutes * 60 seconds/minute = 2700 seconds
Now we can calculate the charge:
Q = 0.5 A * 2700 s = 1350 C
Next, we'll determine the number of moles of electrons transferred using the charge and Faraday's constant:
n = Q / F
Where:
n is the number of moles (mol)
F is Faraday's constant, which is 96500 C/mol
n = 1350 C / 96500 C/mol = 0.014 mol
Now, we can use the stoichiometry of the balanced chemical equation to determine the moles of copper deposited.
The balanced chemical equation for the reduction of copper(II) chloride is:
2CuCl2 + 2e- → 2Cu + 2Cl-
From the equation, we see that 2 moles of electrons are needed to produce 2 moles of copper. Therefore, the moles of copper deposited would be equal to the moles of electrons transferred:
moles of copper = 0.014 mol
Finally, we can calculate the mass of copper using its molar mass.
The molar mass of copper is 63.55 g/mol (which is approximately 63 g/mol).
mass of copper = moles of copper * molar mass of copper
mass of copper = 0.014 mol * 63 g/mol = 0.882 g
Therefore, approximately 0.882 grams of copper would be deposited when a current of 0.5 A was passed through the copper(II) chloride solution for 45 minutes in the electrolytic cell.