Chromium metal can be plated out from an acidic solution containing `CrO_(3)` according to the following equation `:`
`CrO_(3)(aq)+6H^(o+)+6H^(o+)(aq)+6e^(-) rarr Cr(s)+3H_(2)O`
`a.` How many grams of chromium will be plated out by `24000C` ?
`b.` How long will take to plate out `1.5g` of chromium by using `12.5 A` current ?

Explanation

`6XX96500` coulombs deposite `Cr=(52xx24000)/(6xx 96500 )g = 2.1553 g `
(ii) 52 g of Cr is deposit by electricity`=6xx 96500 C`
1.5 g required electricity `=(6xx 96500)/(52)xx1.5 C = 16071 C`
Time for which the current is required to be passed`=(16071.9C)/(12.5 A)=1336 S`