How many grams of silver could be plated out on a serving tray be electrolysis of solution containing silver in `+1` oxidation state for a period of `8.0` hour at a current of `8.46` ampere? What is the area of the tray if the thickness of the silver plating is `0.00254 cm`? Density of silver is `10.5 g//cm^(3)`.

Explanation

Step I. Calculation of the amount of silver deposited.
`Ag^(+)+underset(96500 C)underset(1 mol)(e)^(-)tounderset(108.0 g)underset(1 mol)(Ag)`
Quantity of charge passed (Q)`="current"xx"time"=(8.46 A)xx(8xx60xx60s)=243648 C`
96500 C of electricity deposit Ag=108.0 g
24348 C of electricity deposit Ag`=((108g)xx(243648g))/((96500g))=272.68g`
Step II. Calculationof the area of tray
Volume of silver deposited`=("Mass of silver deposited")/("Density of silver")=((272.68g))/((10.5g cm^(-3)))=25.97 cm^(3)`
Thickness of silver plating =0.00254 cm
`:. " " Area of tray =("Volume")/("Thickness")=((25.97 cm^(3)))/((0.00254 cm))=1.02xx10^(4)cm^(2)`.