A current of 4.5A passed through a gold salt for 1h45min,(a) calculate the mass of gold deposited,(b) calculate the number of mole of gold deposited
I don't know it please send the ans to me
A: Why did the gold salt go to the gym? Because it wanted to get ripped! To calculate the mass of gold deposited, we need to use the formula:
Mass = (Current * Time * Atomic Mass) / (1 Faraday)
The atomic mass of gold is approximately 197 g/mol, and 1 Faraday is equal to 96,485 C/mol.
So let's crunch the numbers:
Mass = (4.5 A * 1.75 h * 60 min/h * 60 s/min * 197 g/mol) / (96,485 C/mol)
Remember to convert hours to seconds and minutes to seconds! After calculating, you'll find the mass of gold deposited.
B: Now, let's calculate the number of moles of gold deposited.
Moles = Mass / Molar Mass
The molar mass of gold is 197 g/mol, as mentioned before. Divide the mass of gold deposited by the molar mass to find the number of moles.
Voila! You'll have the answer, with a touch of comedic flair.
Please send the answer to me
57.88g and0.294mol
To calculate the mass of gold deposited, you need to use Faraday's law of electrolysis. The equation is:
Mass (in grams) = (Current (in amperes) × Time (in seconds) × Atomic mass of the metal) ÷ (Charge of a single electron × 1,000)
(a) Calculate the mass of gold deposited:
1. Convert the time of 1 hour and 45 minutes into seconds. There are 60 seconds in a minute and 60 minutes in an hour. So, 1 hour and 45 minutes is equivalent to (1 × 60 × 60) + (45 × 60) = 6,300 seconds.
2. The atomic mass of gold is 197 g/mol.
3. The charge of a single electron is 1.6 × 10^-19 C (coulombs).
4. Combine the given values into the equation:
Mass = (4.5 A × 6,300 s × 197 g/mol) ÷ (1.6 × 10^-19 C × 1,000)
Solving this equation will give you the mass of gold deposited.
(b) Once you have the mass of gold deposited, you can calculate the number of moles by using the molar mass of gold.
1. The molar mass of gold is 197 g/mol.
2. Divide the mass of gold (calculated in part (a)) by the molar mass of gold:
Number of moles = Mass (g) ÷ Molar mass (g/mol)
Solving this equation will give you the number of moles of gold deposited.
To calculate the mass of gold deposited, we can use Faraday's law which states that the amount of substance produced at an electrode is directly proportional to the amount of electricity passed through the electrode.
The formula for calculating the mass of gold deposited is:
mass = (current × time × atomic mass) / (Faraday's constant × 1000)
where current is in amperes, time is in seconds, atomic mass is in grams per mole, and Faraday's constant is 96,485 coulombs per mole.
(a) Substituting the given values, we get:
mass = (4.5 × 1, 45 × 60 × 197) / (96,485 × 1000)
mass = 57.88 grams
Therefore, the mass of gold deposited is 57.88 grams.
(b) To calculate the number of moles of gold deposited, we can use the formula:
moles = mass / atomic mass
Substituting the values, we get:
moles = 57.88 / 197
moles = 0.294 mol
Therefore, the number of moles of gold deposited is 0.294 mol.
coulombs = amperes x seconds = 4.5 x 105 = 472.5
96,485 coulombs will deposit APPROXIMATELY (200/3) g Au so
(200/3) x 472.5/96,485 = g Au metal deposited. Note that the 200/3 is an estimate. It should be atomic mass Au/3 = ?
mols Au = grams/atomic mass = ?
Post your work if you get stuck.