A current of 156A is applied to an electrolytic cell containing molten CuCl2 for 45 minutes. What substance and how many grams of it will form on the cathode?
Cu^2+ + 2e ==> Cu...........This is gain of electrons; therefore, reduction.
2Cl^- ==> Cl2 + 2e............This is a loss of electrons; therefore, oxidation.
Oxidation occurs at the anode; reduction occurs at the cathod. Therefore, we want the Cu half reaction.
How many coulombs do we generate? That's
Coulombs = amperes x seconds = 146 A x 45 min x (60 sec/min) = 394,200.
1 Faraday or 96,485 coulombs will deposit 63.54 g/2 = 31.77 g Cu metal.
So you can deposit 31.77 g Cu x (394,200/96,485) = ? g Cu
Well, with a current of 156A for 45 minutes, that's quite the shocking situation! It seems like you're all charged up with this question! Let's break it down, shall we?
Now, this electrolytic cell contains molten CuCl2. Copper chloride, eh? Electrolysis involves the decomposition of a compound using electricity. So, we can expect the CuCl2 to be broken down into its constituent elements.
Since Cu2+ ions are positively charged, they will be attracted to the cathode, where they can kick back and relax. These relaxed Cu2+ ions will happily accept a couple of electrons and get converted into copper atoms. Voila!
To determine how many grams of copper will form on the cathode, we need to calculate the amount of charge that has passed through the cell. Given that 1 Coulomb (C) is equivalent to 1 Ampere-second (A·s), we can multiply the current (156A) by the time (45 minutes, or 2700 seconds) to find the total charge.
Once we have the total charge, we can use Faraday's laws to calculate the amount of substance formed. Since Cu2+ requires two electrons to be reduced to Cu, we need to divide the total charge by the charge per mole of electrons (2 x Faraday constant) to find the number of moles of copper formed.
Finally, we can convert moles of copper into grams by multiplying by the molar mass of copper. The molar mass of copper (Cu) is approximately 63.55 grams per mole.
Now, let's crunch those numbers and calculate the grams of copper formed on the cathode. And don't worry, I won't charge you extra for the electricity puns!
But hey, before we get started with the calculations, tell me, does this answer current-ly make sense to you?
To determine the substance and the number of grams formed on the cathode during the electrolysis of CuCl2, we need to first calculate the amount of charge passed through the electrolytic cell using Faraday's Law.
Faraday's Law states that the amount of substance produced or consumed during electrolysis is directly proportional to the amount of electric charge passed through the cell.
1. Calculate the amount of charge passed through the cell:
Charge (Q) = Current (I) x Time (t)
Q = 156A x 45 min
Note: It is important to convert the time to seconds since the unit of charge is Coulombs (C).
1 hour = 60 minutes
1 minute = 60 seconds
Therefore,
Q = 156A x 45 min x (60s/1min)
2. Calculate the number of moles of electrons (n) passed through the cell:
1 mole of electrons = 1 Faraday (F) = 96,500 C
n (in moles) = Q / F
3. Determine the number of moles of Cu deposited on the cathode:
Since Cu2+ ions are reduced to Cu, the number of moles of Cu is equal to the number of moles of electrons.
4. Convert the number of moles of Cu to grams:
Molar mass of Cu = 63.55 g/mol
Now, let's perform the calculations step by step:
Step 1: Calculate the amount of charge passed through the cell:
Q = 156A x 45 min x (60s/1min)
Step 2: Calculate the number of moles of electrons (n) passed through the cell:
n (in moles) = Q / F
Step 3: Determine the number of moles of Cu deposited on the cathode.
Step 4: Convert the number of moles of Cu to grams:
m (in grams) = n x Molar mass of Cu
By following these steps, we can determine the substance and the number of grams formed on the cathode during the electrolysis.
To determine the substance and the number of grams formed on the cathode, we need to calculate the amount of substance deposited using Faraday's laws of electrolysis.
First, we need to determine the number of moles of electrons involved in the electrolysis process.
The current (I) is given as 156A, and the time (t) is given as 45 minutes. However, it is necessary to convert the time into seconds for consistent units.
Given,
Current (I) = 156A
Time (t) = 45 minutes = 45 * 60 seconds = 2700 seconds
Now, let's calculate the number of moles of electrons (n) using Faraday's laws:
n = I * t / F
where:
I = Current in amperes
t = Time in seconds
F = Faraday's constant = 96,485 C/mol e-
n = (156A * 2700s) / 96,485 C/mol e-
n = 4.36 mol e-
According to the stoichiometry of the reaction, for every 2 moles of electrons, 1 mole of copper will be deposited. Therefore, the number of moles of copper formed at the cathode will be half of the number of moles of electrons.
Number of moles of Cu = 4.36 mol e- / 2
Number of moles of Cu = 2.18 mol Cu
Finally, we can determine the mass of copper formed by multiplying the number of moles of copper by its molar mass. The molar mass of copper (Cu) is approximately 63.55 g/mol.
Mass of copper = Number of moles of Cu * Molar mass of Cu
Mass of copper = 2.18 mol Cu * 63.55 g/mol
Mass of copper ≈ 138.271 g
Therefore, approximately 138.271 grams of copper will be formed on the cathode.