An oxide of metal (at . Wt = 112) contains 12.5% of oxygen by weight. What is the valency of metal? What mass of the metal will be liberated when the oxide is converted to chloride with HCl and electrolysed using a current of 9.65 amp for a period of 30 min?

Explanation

Equivalent of oxygen = Equivalent of metal
`12.5/8 = 87.5/E `, where E is the equivalent weight of metal, E= 56
Valency of metal = At. Wt/Eq. wt = `112//56 = 2`
Mass of the metal deposited = `(E xx i xx t)/(96500) = (56 xx 9.65 xx 30 xx 60)/(96500) = 10.08 g`.