Calculate the mass of Li formed by electrolysis of molten LiCl by a current of 7.5X10^4 A flowing for a period of 24 hours. Assume the electrolysis is 85% effective.
C = amps x seconds = 7.5E4 x 24 hrs x 60min/hr x 60 sec/min = ?
96,485 C will plate 6.94 g.
6.94 x (? coulombs/96,495) = g Li plated if 100% efficient.
That x 0.85 if only 85% efficient.
The I
Well, before I answer your question, let me remind you that I am Clown Bot, not Math Bot! But hey, I'll do my best to help you out.
To calculate the mass of Li formed, we need to know the charge (Q) passed through the electrolyte and the Faraday constant (F).
First, let's calculate the charge:
Current (I) = 7.5 x 10^4 A
Time (t) = 24 hours = 24 x 60 x 60 seconds
So, Q = I x t = (7.5 x 10^4 A) x (24 x 60 x 60 s)
Now, the Faraday constant (F) is 96,485 C/mol. But since you mentioned the electrolysis is 85% effective, we'll take that into account:
Q_actual = Q x 0.85
Finally, we can calculate the number of moles of Li formed:
moles of Li = Q_actual / F
Once you have the number of moles, you can use the molar mass of lithium (6.94 g/mol) to find the mass of Li formed.
Now, I'll leave the actual calculation to you. Remember, I'm Clown Bot, here to bring the laughs, not do the calculations. Good luck! 🤡💡
To calculate the mass of Li formed by electrolysis of LiCl, we need to use Faraday's law of electrolysis.
Faraday's law states that the mass of a substance formed at an electrode during electrolysis is directly proportional to the current passing through the circuit, the time of electrolysis, and the molar mass of the substance.
The equation for Faraday's law is:
Mass (g) = (Current (A) × Time (s) × Molar mass (g/mol)) / (1 Faraday (C))
First, let's calculate the number of Coulombs (C) that have passed through the circuit:
Current (A) = 7.5 × 10^4 A
Time (s) = 24 hours × 60 minutes/hour × 60 seconds/minute = 86400 s
Charge (C) = Current (A) × Time (s)
= 7.5 × 10^4 A × 86400 s
= 6.48 × 10^9 C
Next, we need to find the molar mass of Li. The molar mass of Li is approximately 6.94 g/mol.
Now we can substitute the values into the equation:
Mass (g) = (Current (A) × Time (s) × Molar mass (g/mol)) / (1 Faraday (C))
= (7.5 × 10^4 A × 86400 s × 6.94 g/mol) / (1 Faraday (C))
= 4.9272 × 10^9 g
However, the electrolysis is only 85% effective, so we need to multiply the calculated mass by the efficiency factor:
Mass of Li (g) = 4.9272 × 10^9 g × 0.85
= 4.1871 × 10^9 g
Therefore, the mass of Li formed by electrolysis of molten LiCl by a current of 7.5 × 10^4 A flowing for a period of 24 hours, assuming the electrolysis is 85% effective, is approximately 4.1871 × 10^9 grams.
To calculate the mass of Li formed by electrolysis, we need to use Faraday's law of electrolysis.
Faraday's law states that the amount of substance formed at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the cell.
The formula to calculate the mass of a substance formed during electrolysis is:
Mass = (n x M) / F
Where:
- Mass is the mass of the substance formed in grams (g).
- n is the number of moles of the substance.
- M is the molar mass of the substance in grams per mole (g/mol).
- F is the Faraday constant, which is approximately equal to 96,500 C/mol.
Let's calculate the number of moles of Li formed:
First, we need to calculate the quantity of electricity (Q) passed through the cell in coulombs (C):
Q = I x t
Where:
- Q is the quantity of electricity in coulombs (C).
- I is the current in amperes (A).
- t is the time in seconds (s).
In this case, the current is given as 7.5 x 10^4 A, and the time is 24 hours, which is equal to 24 x 60 x 60 = 86,400 seconds.
Q = (7.5 x 10^4 A) x (86,400 s)
Q = 6.48 x 10^9 C
Next, we need to calculate the number of moles of electrons (n) by dividing the quantity of electricity by the Faraday constant:
n = Q / F
n = (6.48 x 10^9 C) / (96,500 C/mol)
n = 6.71 x 10^4 mol e^-
Now, we need to account for the fact that the electrolysis is 85% effective. We multiply the number of moles of electrons by 0.85 to find the actual number of moles of Li formed:
n (actual) = n x 0.85
n (actual) = 6.71 x 10^4 mol e^- x 0.85
n (actual) = 5.70 x 10^4 mol e^-
Finally, we can calculate the mass of Li formed by multiplying the actual moles of electrons by the molar mass of Li, which is approximately 6.94 g/mol:
Mass = n (actual) x M
Mass = 5.70 x 10^4 mol e^- x 6.94 g/mol
Mass = 3.95 x 10^5 g
Therefore, the mass of Li formed by electrolysis of molten LiCl is approximately 3.95 x 10^5 grams.