If the current is used, find the time taken for 5.5kg of gold to be deposited (Au = 197, 1 faraday = 96500c)
To find the time taken for 5.5 kg of gold to be deposited, we need to use Faraday's law of electrolysis:
m = ZIt / F
Where:
m = mass of the substance deposited (in grams)
Z = electrochemical equivalent (in g/C)
I = current (in amperes)
t = time (in seconds)
F = Faraday constant (in C/mol)
First, let's convert the mass from kg to grams:
m = 5.5 kg * 1000 = 5500 g
Next, we need to calculate the number of moles of gold:
moles = mass / molar mass
moles = 5500 g / 197 g/mol = 27.92 mol
Now, we can find the electrochemical equivalent (Z):
Z = molar mass / F
Z = 197 g/mol / 96500 C/mol = 0.002039 g/C
Finally, we can rearrange the equation and solve for time (t):
t = m / (Z * I / F)
t = 5500 g / (0.002039 g/C * I / 96500 C/mol)
Assuming the current (I) is given, you can substitute its value into the equation above to find the time taken for gold to be deposited.