Posted by Chopsticks on Wednesday, January 21, 2009 at 6:04pm.
Determine the simplest formula for compounds that have the following analyses. The data may not be exact.
28.5% iron, 48.6% O, 22.9% S
This is what I did:
28.5g Fe 1 mole Fe/55.847g = .51 mole
48.6g O 1 mole O/15.999g = 3.04 mole
22.9g S 1 mole S/32.064g = .71 mole
(Fe1.0 O6.0 S1.4)5 = Fe5 O30 S7
is that right? can you please help me check my answer?
Chemistry - bobpursley, Wednesday, January 21, 2009 at 6:20pm
The thing that strikes me is the sum of the compositions is exactly 100 percent, yet the problem says it may not be exact. So if Fe were reduced by .6gram, and S were increased by .6 gram. ... one gets Iron(II) sulfite
Chemistry - Chopsticks, Wednesday, January 21, 2009 at 6:55pm
I don't get it either. But overall, did i get my calculation right? or did i do the process right?
Chemistry - DrBob222, Wednesday, January 21, 2009 at 7:36pm
The process looks ok to me. The statement about not being exact but the percentages add to 100.0 (plus few of us have heard of Fe5S7O30)makes me think that the problem was made up.
Chemistry - Chopsticks, Wednesday, January 21, 2009 at 9:07pm
yea they are completely made up.
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