How many grams of silver could be plated out on a serving tray by electrolysis of a solution containing `Ag^(+)` for a period of 8.0 h at a current of 8.46 A. What is the area of tray if the thickness of Ag-plating is `"0.00254 cm"`? Density of `"Ag = 10.5 g.cm"^(-3)`.

Explanation

The quantity of electricity sent `=8.46xx(8xx3600)C=243648C`
`Ag^(+)(aq)+underset("24648C")underset("96500C")(e)rarr underset("272.68g")underset("108g")(Ag)`
So, 272.68 g of Ag could be plated out.
Volume of `"272.68g of Ag"=(272.68)/("density")=(272.68)/(10.5)cm^(3)`
`=25.97cm^(3)`
If area of the tray of `"A cm"^(2)`, then
`Axx` its thickness `=25.97" or, "A=(25.97)/(0.00254)=25.97`
Therefore, area of the tray = `"10224.4 cm"^(2)`.