Two voltameters, one having a solution of silver salt and the other of a trivalent-metal salt, are connected in series and a current of `2 A` is maintained for `1.50 hours`. It is found that `1.00 g` of the trivalent metal is deposited. (a) What is the atomic weight of the trivalent metal? (b) How much silver is deposited during this period?
Atomic weight of silver is `109.9 g mol^(-1)`

Explanation

`m = (Eit)/(F)`
`E = A/V = A/3`
`m = (Ait)/(3F) `
`1=(Axx2xx1.5xx3600)/(3xx96500) implies A = 26.8g//"mole"`
(b) `m = (Eit)/(F) =(107.9xx2xx1.5xx3600)/(96500)`
`=12.1g`.