What weight of silver is obtained during the electrolysis when same quantity of electricity deposits 18 grams of Aluminium? (Atomic mass of Silver is 108)

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

0.02 equivalent of Ag was deposited in an electrolysis experiment. If same quantity of a electricity is passed through a gold solution, 1.314 g of gold is deposited. Find oxidation state of the gold. (Atomic mass of Au = 197)

The weight of silver (at wt. = 108 ) displaced by a quantity of electricity which displaced 5600 mL of O_(2) at STP will be:

What weight of Ni is plated out in an electrolysis of aqueous NiSO_(4) solution that it takes place to deposit 2G OF Ag in a silver coulometer that is arranged in series with NiSO_(4) electrolytic cell. [ Atomic weight of Ag=107.8 am u , atomic weight of Ni=58.7 am u]

The quantity of electricity needed to liberate 0.5 gram equivalent of an element, during electrolysis is

25 gm of a metal is deposited on cathode during the electrolysis of metal nitrate solution by a current of 5 apm pssing for 4 hour if atomic weight of the metal is 100 The valency of metal in metal intrates is

Assertion : In electrolysis, the quantity of electricity needed for depositing 1 mole silver is different from that required for 1 mole of copper. Reason : The molecular weights of silver and copper are different.

19 g of molten SnCl_2 is electrolysed for sometime using inert electrodes. 0.119g of Sn is deposited at the cathode. No substance is lost during the electrolysis. The ratio of the weights of SnCl_2 : SnCl_4 after electrolysis [Atomic weight of Sn = 119 ]

Salts of A (atomic weight 7 ), B (atomic weight 27 ) and C (atomic weight 48 ) were electolysed under idential condition using the same quanity of electricity. It was found that when 2.1 g of A was deposited, the weights of B and C deposited were 2.7 and 7.2 g . The valencies A, B and C respectively: