The amount of electricity required to deposit 1.0 mole of aluminium from a solution of `AlCl_(3)` will be

Calculate the amount of electricity required to deposite 0.9 g of aluminium by electrolysis of a salt containing its ion, if the electrode reaction is Al^(3+)+3e^(-)rarrAl , (atomic mass of Al =27, 1F=96500C )

The number of electrons required to deposit 1g equivalent aluminium (At. Wt. =27) from a solution of aluminium chloride will be

The amount of electricity that can deposit 108g of silver from silver nitrate solution is

The quantity of charge required to obtain one mole of aluminium from Al_(2)0_(3) is

The quantity of charge required to obtain one mole of aluminium from Al_(2)0_(3) is

How many faradays of eletricity is required to deposit 2 mole copper from CuSO_(4) solution

The quantity of electricity required to deposit 1*15g of sodium from molten NaCl (Na = 23, Cl = 35*5) is

1 C electricity deposits:

Answer the following questions : Calculate the number of coulombs required to deposit 20.25 g of aluminium (at. mass = 27) from a solution containing Al^(+3)

The quantity of electricity required to reduce 0.5 mole of (MnO_(4))^(1-) to Mn^(2+) is