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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 the reaction:
`CrO_(3) + 6H^(+) + 6e^(-) rarr Cr + 3H_(2)O`
How long will it take to plate out 1.5 gm of Cr using 12.5 ampere current ? (Atomic weight of Cr =52, 1F =96500 C)

Text Solution

Verified by Experts

`Cr O_(3) (aq) + 6 H^(+) (aq) + 6e^(-) to Cr (s) + 3 H_(2)O`
Since 6 mole of electrons are required to deposit 1 mol of Cr
Amount of electricity needed to plate out 1 mol Cr (52 g ) = `96500 xx 6` C
Amount of electricity required to deposit 1.5 g of Cr =` (96500 xx 6)/(52) xx 1.5 = 16071.9 ` C
Time for which electricity is to be passed ,
`Q = I xx t`
`16071.9 = 12.5 xx t`
`t = (16071.9)/(12.5) = 1336.15s`
t = 22.27 min .
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