The current of 2 A is passed for 5 h through a molten tin salt to deposit 22.2 g tin. What is the oxidation state of tin in salt? [Atomic weight of `Sn=118.69 g`]

A current of 2.0 ampere is passed for 5.0 hour through a molten tin salt to deposit 22.2 g tin. What is the oxidation state of tin in salt? Atomic wt. of Sn = 118.69 g .

If 2 A current passes for 5 h through a molten tin salt to deposit 22.2 g tin, what will be the oxidation number of tin in the salt? [At. Mass of tin = 118.7]

A current of 2 ampere passing for 5 hr through a molten tin salt deposits 22.2 g of tin. Find the oxidation number of tin (atomic weight of tin is 118.7) in the salt

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

A current of 2A is passed for 1.93 xx 10^(4)s through a molten tin salt depositing 23.8 g Sn (Aw of Sn=119) . The oxidation state of Sn in the salt is ………………………… .