How many grams of silver could be plated out on a serving tray by the electrolysis of a solution containing silver in `+1` oxidation state of a period of 8.0 h at a current of 8.46 A ? What is the area of the tray, if the thickness of the silver plating is 0.0254 cm?
`["The density of silver is 10.5 g.cm"^(-3)]`

Explanation

Charges passed through the cell `=8.46xx3xx3600="243648 coulombs"`
Electrode reaction : `Ag^(+)(aq)+e rarr Ag(s)" …[1]"`
`"243648 coulombs "-=(243648)/(96500)-="2.524 mol of electrons"`
According to equation (1) 2.524 mol of electrons
`=180xx2.524="272.6 g of Ag"`
`therefore" Volume of Ag plated out "=(W)/("density")=(272.68)/(10.5)="25.969 cm"^(3)`
Given, thickness of the Ag plating = 0.0254 cm
`therefore" Area of tray plated "=(25.969)/(0.0254)=1022.4=1.02xx10^(3)cm^(2)`