Calculation of Aluminium Deposited:
- Given current = 10 A
- Time = 5 minutes = 300 seconds
- Atomic mass of Aluminium = 27 g/mol
- Charge on 1 mole of Aluminium ions = 3e (where e is the charge of an electron)
1. Calculate the amount of charge passed:
Q = I * t
Q = 10 A * 300 s
Q = 3000 C
2. Calculate the number of moles of Aluminium ions deposited:
Number of moles = Q / (3e)
Number of moles = 3000 C / (3 * 1.6 x 10^-19 C)
Number of moles = 6.25 x 10^18 mol
3. Calculate the mass of Aluminium deposited:
Mass = Number of moles * Atomic mass
Mass = 6.25 x 10^18 mol * 27 g/mol
Mass = 1.69 x 10^20 g

Time taken to deposit 1.08g of Silver:
- Given mass of Silver = 1.08 g
- Atomic mass of Silver = 108 g/mol
- Charge on 1 mole of Silver ions = 1e (where e is the charge of an electron)
1. Calculate the number of moles of Silver ions:
Number of moles = Mass / Atomic mass
Number of moles = 1.08 g / 108 g/mol
Number of moles = 0.01 mol
2. Calculate the amount of charge required:
Q = Number of moles * 1e
Q = 0.01 mol * 1.6 x 10^-19 C
Q = 1.6 x 10^-21 C
3. Calculate the time taken to deposit 1.08g of Silver:
Time = Q / I
Time = 1.6 x 10^-21 C / 10 A
Time = 1.6 x 10^-22 s
Therefore, it will take 1.6 x 10^-22 seconds to deposit 1.08g of Silver.