How much quantity of electricity in coulomb is required to deposit `1.346xx10^(-3)kg` Ag in 3.5 minutes from `AgNO_(3)` solution ? (Given : Molar mass of Ag is `108xx10^(-3) kg "mol"^(-1)`)

Explanation

Given,
Mass of Ag deposit `=1.346xx10^(-3)kg`
`=1.346g`
Time `=3.5` min, `xx60`
`=210` sec.
Molar of mass of Ag `=108xx10^(-3)kg "mol"^(-1)`
`=108 g "mol"^(-1)`
Quantity of electricity `(Q)=?`
Formula,
Mass of Ag`=(Q)/(F)xx`Mole ratio `xx` Molar mass
`:'` Mole ratio of `Ag=Ag^(+)+e^(-)rarr Ag=1/1 = 1`
`:.1.346=(Q)/(96500)xx1xx108`
`Q=(1.346xx96500)/(108)`
`=1202.67C`.
Quantity of electricity required is 1202.67 Coulomb.