Introduction to Combustion Analysis, Empirical Formula & Molecular Formula Problems

This chemistry video tutorial explains how to find the empirical formula and molecular formula using combustion analysis. It explains how to calculate the number of moles of each element given the mass in grams of CO2 and H2O. Examples include compounds containing Carbon, Hydrogen, and Oxygen. This video contains plenty of practice problems
Introduction to Moles:
• Introduction to Moles
How To Calculate The Molar Mass:
• How To Calculate The M...
How To Convert Grams to Moles:
• How To Convert Grams T...
How To Convert Moles to Grams:
• How To Convert Moles t...
Moles to Atoms Conversion:
• Moles To Atoms Convers...
Grams to Molecules Conversion:
• Grams to Molecules and...
_________________________________
Grams to Atoms:
• How To Convert Grams t...
Moles, Atoms, & Grams Conversions:
• How To Convert Between...
How To Balance Chemical Equations:
• How To Balance Chemica...
Stoichiometry - Basic Introduction:
• Stoichiometry Basic In...
Avogadro's Number:
• Avogadro's Number, The...
_________________________________
Limiting Reactant Problems:
• Limiting Reactant Prac...
Excess Reactant Problems:
• How To Find The Amount...
Theoretical & Percent Yield:
• How To Calculate Theor...
Percent Yield - More Examples:
• How To Calculate The P...
Percent Error:
• Percent Error Made Easy!
_________________________________
Percent Composition By Mass:
• Percent Composition By...
Empirical Formula Problems:
• Empirical Formula & Mo...
Empirical Formula - Hydrated Compounds:
• How To Find The Empiri...
Combustion Analysis:
• Introduction to Combus...
Stoichiometry Practice Test:
• How To Solve Stoichiom...
_______________________________________
Final Exams and Video Playlists:
www.video-tutor.net/
Full-Length Videos and Worksheets:
/ collections

[@TheOrganicChemistryTutor]

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[@BrianErwin]

8:50, should explain why you're converted to grams (since you'll need it to calculate oxygen later on), cos as is, you get .188, which you end up getting later in the video, 11:51. same with hydrogen, 10:05, explain that we need this to calculate oxygen, since as is, you end up getting .501 12:19

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[@Jimmy_Vee]

A simpler way to figure out the empirical formula would be to find the composition percentage of carbon in carbon dioxide and hydrogen in dihydrogen monoxide (H2O).
Then, divide the percentages by 100 so that you can then multiply that number by the amount of mass that is given for CO2 and H2O
Then, you'll have the amount of grams of carbon and the amount of grams of hydrogen.
To convert grams to moles just use the formula; number of moles=mass/molar mass. So, divide the amount of grams of carbon by the molar mass of carbon and divide the amount of grams of hydrogen by the molar mass of hydrogen.
Now you have the quantities of both carbon and hydrogen in moles.
Next, divide both mole values by the smaller one. The answer you get will be your coefficient for that element within the compound.
If even one of your coefficients is not a whole number, keep on doing trial and error by multiplying that decimal number by two, then three, then four, and so on until you get a whole number.
If you end up with something like 11.9 after doing trial and error, you can simply round that to 12. If u get something like 11.1, round that to 11. If u get something like 11.2, 11.3, 11.4, 11.5, 11.6, 11.7, or 11.8, you would have to multiply both the coefficients for carbon and hydrogen by a factor that would make that decimal number a whole number. For example, 11.8×5=59✔️
Then you can write out your empirical formula with your obtained coefficients.
Now if you want the molecular formula from this, use the formula molecular formula factor=mass of compound (always given)/empirical molar mass. If you've done it right, you should always get a whole number for this factor.
Simply multiply your coefficients by that factor and now you have your molecular formula as well.
Thank you for coming to my ted talk hehe, have a great day!

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What if we get a decimal instead of a while number after deciding the Molecular Formula Mass by the Empiracle formula mass?

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[@nasreenali1763]

at 10:16 why did you take the mass of hydrogen only 1.008 whereas, we have 2 mols of Hydrogen???But, I still want to say thank you for explaining everything so well.

[@dannylim834]

Hi. I hope my one-year-too-late explanation finds you well. We only take the mass of 1.008 since that's the grams per one mole of hydrogen. We did this to convert our moles to grams.

[@SM-qn7sr]

1 mol of hydrogen is 1.008 and we want to cancel the moles of H to get grams of H

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What happends when i get 1.15 as a result for one of the elements?

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In first problem we didn't × atomic mass / 1 mole of (c, h , o ) but in second one we did why ?. explain please ?
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