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November 08, 2025, 04:21:08 pm
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Author Topic: Understanding mole calculations  (Read 690 times)  Share 

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America

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Understanding mole calculations
« on: April 10, 2013, 03:20:34 pm »
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Hey guys,

This question has been pestering me recently; A pure hydocarbon is burnt in oxygen. The products are carbon dioxide (1.76g) and water (1.08). The empirical formula of the hydrocarbon is

A. CH2
B. CH3
C. C2H3
D. CH4

I don't understand the molar calculations when it comes to finding the C and H from the CO2 and H2O. Many thanks.
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Conic

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Re: Understanding mole calculations
« Reply #1 on: April 10, 2013, 05:38:50 pm »
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Find the amount of carbon and hydrogen, then you can use the usual method of finding the empirical formula.



« Last Edit: April 10, 2013, 05:41:58 pm by Conic »
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2012-13: VCE at Parade College (Chemistry, English, Mathematical Methods, Physics and Specialist Mathematics).
2014-16: Bachelor of Science at La Trobe University (Mathematics and Statistics).
2017-17: Bachelor of Science (Honours) at La Trobe University (Mathematics).
2018-21: PhD at La Trobe University (Mathematics).
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