To calculate the amount of electricity required to deposit 1 mole of metal from a given electrolyte, we need to utilize Faraday's laws of electrolysis. According to Faraday's laws, the amount of substance deposited or liberated at an electrode is directly proportional to the quantity of electricity passed through the electrolyte.

The formula to calculate the amount of electricity required is given by:

Electricity (Coulombs) = (mole of substance) x (Faraday's constant)

1. Electrolyte: AgNO3 (Silver Nitrate)
- The balanced equation for the deposition of silver from silver nitrate is:
Ag+ + e- → Ag
- The number of moles of silver required is 1.
- The Faraday's constant is approximately 96,500 C/mol.
- Therefore, the amount of electricity required is:
Electricity = 1 x 96,500 C

2. Electrolyte: FeSO4 (Iron(II) Sulfate)
- The balanced equation for the deposition of iron from iron(II) sulfate is:
Fe2+ + 2e- → Fe
- The number of moles of iron required is 1.
- The Faraday's constant is approximately 96,500 C/mol.
- Therefore, the amount of electricity required is:
Electricity = 1 x 96,500 C

3. Electrolyte: MgCl2 (Magnesium Chloride)
- The balanced equation for the deposition of magnesium from magnesium chloride is:
Mg2+ + 2e- → Mg
- The number of moles of magnesium required is 1.
- The Faraday's constant is approximately 96,500 C/mol.
- Therefore, the amount of electricity required is:
Electricity = 1 x 96,500 C

4. Electrolyte: CuSO4 (Copper(II) Sulfate)
- The balanced equation for the deposition of copper from copper(II) sulfate is:
Cu2+ + 2e- → Cu
- The number of moles of copper required is 1.
- The Faraday's constant is approximately 96,500 C/mol.
- Therefore, the amount of electricity required is:
Electricity = 1 x 96,500 C

5. Electrolyte: Al2(SO4)3 (Aluminum Sulfate)
- The balanced equation for the deposition of aluminum from aluminum sulfate is:
2Al3+ + 6e- → 2Al
- The number of moles of aluminum required is 1.
- The Faraday's constant is approximately 96,500 C/mol.
- Therefore, the amount of electricity required is:
Electricity = 1 x 96,500 C

In summary, the amount of electricity required to deposit 1 mole of metal from the given electrolytes is 96,500 Coulombs for all the electrolytes mentioned.