How many grams of silver could be plated out of a shield by electrolysis of a solution containing `Ag^(+)` ions for a period of 4 hours at a current strength of 8.5 amperes ?

Explanation

Quantity of charge (Q) passed `=1xxt=(8.5 " amp")xx(4xx60xx60s)`=122400 C
The electrode reaction is :
`{:(Ag^(+)+e^(-)rarrAg),(" "1 mol " "1 mol),(" "96500 C " "107.8 g):}`
96500 C charge can plate out silver =107.8 g
122400 C charge can plate out silver `=((107.8g))/((96500 C))xx(122400 C)`
=136.73 g