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Topic: Electrolyzing a solution  (Read 1479 times)

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Offline magnus

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Electrolyzing a solution
« on: January 27, 2019, 05:10:09 PM »
Hi I have a problem with this:
Electrolyzing a solution of a ruthenium sale for 500 seconds with a current of 120 mA deposited 31.0 g of metallic ruthenium. How much is the
oxidation number of ruthenium in the salt used?

i=Q/t => Q=0.12*500= 60 C

m=Q/F * PM/z  =>  z=Q*PM / F*m = 0.002  ???

The result is impossible... >:( >:(
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Offline Borek

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Re: Electrolyzing a solution
« Reply #1 on: January 27, 2019, 06:19:47 PM »
Are you sure it is 31 g, and not 31 mg?
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Offline magnus

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Re: Electrolyzing a solution
« Reply #2 on: January 28, 2019, 02:43:28 AM »
the text of the question reported those quantities, but I do not think they are real
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Offline Enthalpy

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Re: Electrolyzing a solution
« Reply #3 on: January 28, 2019, 08:45:27 AM »
Either 31mg and 120mA, or 31g and 120A. Or even 500ks.

Don't laugh. Some publications do use ks rather than hours and months. I saw "3.6ks" recently in a metallurgy paper.
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Offline sjb

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Re: Electrolyzing a solution
« Reply #4 on: January 28, 2019, 08:53:43 AM »
Quote from: Enthalpy on January 28, 2019, 08:45:27 AM
Some publications do use ks rather than hours and months. I saw "3.6ks" recently in a metallurgy paper.

Makes the maths easier :)
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