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 `8.0h` at a current of `8.46A` ? What is the area of the ray, if the thickness of the silver plating is `0.0254 cm` ? The density of silver is 10.5 g cm^(-3)`.

Answer

`272.68g,1.02xx10^(4)cm^(2)`

Explanation

Using the expression
`m=ZxxQ`
`Z=(Aw)/(F):`
`=(Aw)/(F)xxIxxt(` due to `+1` oxidation state of silver salt `)`
`=(108)/(96500)xx8.46xx8xx60xx60g`
`=272.68g(:'8h=8xx60xx60s)`
Volume of silver placed out `(V)=(m)/(d)=(272.68g)/(10.5g cm^(-3))`
Area of the tray plated `=(25.969 cm^(3))/(0.00254cm)`
`=10224.2cm^(2)=1.02xx10^(4)cm^(2)`