If the current is used, find the time taken for 5.5g of gold to be deposited ( Au =197, 1 faraday = 96500c )
To calculate the time taken for 5.5g of gold to be deposited, we need to use Faraday's law of electrolysis.
Faraday's law states that the amount of substance deposited or liberated at an electrode during electrolysis is directly proportional to the quantity of electricity passed through it.
The formula is:
Amount of substance (in moles) = (Electric charge)/(Faraday's constant)
First, we need to calculate the number of moles of gold that will be deposited.
The molar mass of gold (Au) is 197g/mol.
So, the number of moles of gold can be calculated as:
Number of moles = (Mass of gold)/(Molar mass of gold)
Number of moles = 5.5g / 197g/mol
Number of moles = 0.02792 mol
Now, we need to calculate the electric charge required to deposit this amount of gold.
The formula is:
Electric charge (in coulombs) = (Number of moles) * (Faraday's constant)
Electric charge = 0.02792 mol * 96500 C/mol
Electric charge = 2694.98 C
Finally, we can calculate the time taken using the formula:
Time (in seconds) = (Electric charge)/(Current)
We need to know the current to calculate the time.