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Chromium metal can be plated out from an...

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 ?

Text Solution

Verified by Experts

`CrO_(3)+6H^(+)+underset(6xx96500 C)(6e^(-)) rarr underset(("1 mole"),(52 g))(Cr)+3H_(2)O`
Mass of chromium plated out by 24000 coulomb charge
`=52/(6xx96500)xx24000=2.155 g`
Charge required for plating out 1.5 g of chromium
`=(6xx96500)/52xx1.5=16701.92` coulomb
Time=`("Charge")/("current")=16701.92/12.5=1336.15` second
`=22.27` minute
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