The density of copper is `8.95 g mL^(-1)`. Find out the number of coulombs needed to plate an area of `100cm^(2)` to a thickness of `10^(-2)cm` using `CuSO_(4)` solution as electrolyte. `(` Atomic weight of `Cu=63.5g)`

Explanation

Volume of `Cu^(2+)` ion deposited on plate `(` Area `xx` thickness `)`
`=100cm^(2)xx10^(-2)cm`
`=1cm^(3)`
Weight of `Cu^(2+)` deposited `=` Volume `xx` Density
`=1cm^(3_xx8.95g mL^(-1)`
`=8.95g`
Now,`Cu^(2+)+2e^(-)rarr Cu`
First method
`2e^(-)=2F-=1 mol ` of `Cu=63.5g `of `Cu`
`-=2F`
`-=2xx96500C`
`:. 8.95g `of `Cu=(2xx96500xx8.95)/(63.5)`
`=27202.36C`
Or use direct formula
`W=(E_(w)xxI(A)xxtsec)/(96500),,,,,,,( :'Q=It)`
`8.95=(63.5//2xxQ)/(96500)impliesQ=27202.36C`
Second method
`1F=1Eq` of `Cu`
`=(63.5)/(2)g `of `Cu`
`(63.5)/(2)g` of `Cu=96500C`
`:. 8.95g` of `Cu=(96500xx2xx8.95)/(63.5)`
`=27202.36C`