A current of 45A is passing through a solution of gold salt for 1:45 minutes
a)calculate the mass of AU deposited
b )number of mass deposited
c) if the same current is use find the time taken for 5.5 g of the AU deposited
Please where did you get the 96,485 from.
How is it 96485 and where did the 197/3 come from
coulombs = amperes x seconds or
coulombs = 45 x 1.75 hrs x (60 min/hr) x (60 sec/min) = 283,500
96,485 coulombs will deposit about 197/3 g Au But you can use closer numbers than that.
So g Au deposited = (197/3) x (283,500/96,485) = ? g Au.
I suppose part b is mols and not mass so g Au/molar mass = mols Au.
C. Follow the steps in part A to do C and find the time.
Post your work if you get stuck.
what the correct answer?
a) Well, there's only one way to find out the mass of AU deposited - ask it politely! "Hey AU, how much do you weigh?" Just kidding! Sorry for the confusion. To calculate the mass of AU deposited, we need to use a bit of chemistry magic. We first need to know the molar mass of AU. Sure, gold might be heavy, but does it ever go on a diet? The molar mass of gold (AU) is roughly 197 grams per mole.
Now, let's convert the amount of charge passed into the number of moles of gold. We know that 1 Faraday (F) is equal to 96,485 Coulombs (C). So, we divide the amount of charge passed (45 Amperes x 1.75 minutes x 60 seconds) by the Faraday constant to get the number of moles of gold deposited.
Next, we multiply the moles of gold by the molar mass of gold to find the mass of AU deposited.
b) The number of moles of gold deposited is the same as the answer to part (a). Convenient, right? It's like killing two birds with one calculator!
c) To find the time taken for 5.5 grams of AU to be deposited at the same current, we need to reverse the previous calculations. First, divide the mass of AU (5.5 g) by its molar mass to get the number of moles. Next, multiply the number of moles by the Faraday constant (96,485 C) to convert it into charge. Finally, divide the charge by the current of 45A to get the time taken in seconds.
Hope that answers your questions! Remember, don't take Gold's weight personally. It's just Au-niversal!
To calculate the mass of gold deposited, we need to use Faraday's Law of Electrolysis. This law states that the mass of a substance deposited during electrolysis is directly proportional to the charge passed through the electrolyte.
a) Calculate the mass of gold deposited:
1. Determine the charge passed through the solution. Charge (Q) = Current (I) x Time (t).
Q = 45A x (1 hour 45 minutes)
= 45A x (1 hour + 45/60 hours)
= 45A x (1.75 hours)
= 78.75 Coulombs
2. Find the Faraday's constant (F). The value of F is the charge carried by one mole of electrons and is equal to 96,485 Coulombs per mole.
3. Calculate the number of moles of gold deposited using the equation:
Moles of gold (n) = Charge (Q) / Faraday's constant (F)
n = 78.75 C / 96,485 C/mol
n = 0.000816 moles
4. Determine the molar mass of gold (Au) which is approximately 197 g/mol.
5. Calculate the mass of gold deposited using the equation:
Mass (m) = Moles of gold (n) x Molar mass of gold (M)
m = 0.000816 moles x 197 g/mol
m = 0.160 g
Therefore, the mass of gold deposited is 0.160 g.
b) To determine the number of moles of gold deposited, we can directly use the result from step 3, which is 0.000816 moles.
c) If the same current is used, and we need to find the time taken for 5.5 g of gold to be deposited, we use the equation:
Moles of gold (n) = Mass of gold (m) / Molar mass of gold (M)
Rearranging the equation to solve for time (t):
Time (t) = Moles of gold (n) * Molar mass of gold (M) / Current (I)
Plugging in the given values:
t = (5.5 g / 197 g/mol) / 45A
Calculating the time:
t ≈ 0.063 hours or about 3.78 minutes.
Therefore, it would take approximately 3.78 minutes for 5.5 g of gold to be deposited with the same current.