A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes `FeSO_(4) and ZnSO_(4)` until 2.8 g of Fe deposited at the cathode of cell X. How long did the current flow? Calculate the mass of Zn deposited at the cathode of cell Y.
(Molar mass : `Fe=56 g"mol"^(-1)Zn=65.3"g mol"^(-1), F=96500"C mol"^(-1)`)

Explanation

`m=z I t`
`2.8g=(56xx2xx t)/(2xx96500)`
`t=4825s`
`(m_(1))/(m_(2))=(E_(1))/(E_(2))`
`(2.8)/(mZn)=(56)/(2)xx(2)/(65.3)`
`mZn=3.265g`