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# Empirical Formula Watch

1. How do I work out the empirical formula of the compound CH0.22O0.46? Randomly guessing ratios isn't going to work out ...
How do I work out the empirical formula of the compound CH0.22O0.46? Randomly guessing ratios isn't going to work out ...
Divide each component by the smallest ratio (in this case 0.22)

This gives: C:4.55; H:1; O:2.09

At this stage I would look for a factor that would make the smallest non-integral number into an integer.

It's useful at this point to know the first few fractions off by heart. For example, I recognise the decimal 0.0909 as being 1/11. So I would then multiply everything be 11.

C:50, H:11, O:23

I haven't a clue as to the identity of this molecule by the way ...
3. (Original post by charco)
Divide each component by the smallest ratio (in this case 0.22)

This gives: C:4.55; H:1; O:2.09

At this stage I would look for a factor that would make the smallest non-integral number into an integer.

It's useful at this point to know the first few fractions off by heart. For example, I recognise the decimal 0.0909 as being 1/11. So I would then multiply everything be 11.

C:50, H:11, O:23

I haven't a clue as to the identity of this molecule by the way ...
Thank you!

It's not a molecular formula but rather the net formula of a covalent lattice - graphite oxide, according to the Lerf-Klinowski model. It's the first broad problem you can find here: http://icho2013.chem.msu.ru/material..._IChO_2013.pdf

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Updated: March 28, 2013
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