A currrent of 5.0 A flows for 4.0 h through an electrlytic cell containing a molten salt of metalM. This results in deposition of 0.25 mol of the metal M at the cathode. The oxidation state of M in the molten salt is : (1 Faraday=`96485 C "mol"^(-1)`)

A current of 5.0 A flows for 4.0 h through an electrolytic cell containing a molten slat of metal M. This result in deposition of 0.25 mol of the metal M at the cathode. The oxidation state of M in the molten salt is +x . The value of 'x' is (1 Faraday = 96000 C mol^(-1) )

A current of 5.0 A flows for 4.0 h through an electrolytic cell containing a molten slat of metal M. This result in deposition of 0.25 mol of the metal M at the cathode. The oxidation state of M in the molten salt is +x . The value of 'x' is (1 Faraday = 96000 C mol^(-1) ) 3

A current of 2.0A passed for 5 hours through a molten metal salt deposits 22.2 g of metal (At. Wt. =177). The oxidation state of the metal in the metal salt is

A current of 2.0A passed for 5 hours through a molten metal salt deposits 22.2 g of metal (At. Wt. =177). The oxidation state of the metal in the metal salt is

What amount of electricity can deposit 1 mol of Al metal at cathode when passing through molten AlCl_(3) -

When 6 xx 10^22 electrons are used in the electrolysis of a metallic salt, 1.9 gm of the metal is deposited at the cathode. The atomic weight of that metal is 57. So oxidation state of the metal in the salt is