If the current is used, find the time taken for 5.5g of gold to be deposited (Au = 197, 1 faraday = 96500c )
To find the time taken for 5.5g of gold (Au) to be deposited, we need to use Faraday's law of electrolysis.
The formula to calculate the amount of substance deposited during electrolysis is:
n = Q / (z * F)
Where:
n = amount of substance (in moles)
Q = total electric charge (in coulombs)
z = number of moles of electrons transferred per mole of substance
F = Faraday's constant (96500 C/mol)
First, we need to calculate the number of moles of gold (Au) using its molar mass:
molar mass of Au = 197 g/mol
mass of gold (Au) = 5.5 g
n = (5.5 g) / (197 g/mol)
n = 0.0279 moles
Now, we need to find the total electric charge (Q) required to deposit this amount of gold. Since gold has a charge of +3 (Au^3+ to Au), z = 3:
n = Q / (z * F)
0.0279 moles = Q / (3 * 96500 C/mol)
Q = 0.0279 moles * 3 * 96500 C/mol
Q = 8052.45 C
Finally, we can calculate the time taken using the equation:
Q = I * t
where:
I = current (in Amperes)
t = time (in seconds)
Assuming we have a constant current, we can rearrange the equation to solve for time:
t = Q / I
If we assume I = 1 Ampere, then:
t = 8052.45 C / 1 A
t = 8052.45 s
Therefore, the time taken for 5.5g of gold to be deposited using a current of 1 Ampere is approximately 8052.45 seconds.