Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: toffeefan on September 03, 2009, 10:56:50 AM
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Consider the following equation (I know the equation is not balanced, its just a random example I've created):
5C2H4O + 2H2 :rarrow: 3C2H6O
A gaseous mixture consisting of 50 mol% H2 and 50 mol% C2H4O before a reaction was 5 moles. After reaction, it was found that the total number of moles left was 2. Here is the mole balance I've created, is it correct?
Moles of C2H4O left + Moles of H2 left + Moles of C2H6O produced = 2 mol (total moles left)
(2.5mol - 5x) + (2.5mol - 2x) + 3x = 2 moles
3 3
Where X = mol of C2H6O produce.
I'm not sure if the mole balance is correct, especially the 3x part. Can somebody please clarify? Thanks.
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Hi,
I posted this on another forum and it got locked. There is no answer for this, it's just an example i created. All i want to know is weather the method i set up for this mole balance is correct.
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As far as I can tell at 0:20 am it looks OK.