October 18, 2024, 04:55:25 AM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Determining Empirical Formula  (Read 5988 times)

0 Members and 1 Guest are viewing this topic.

kissoftalons

  • Guest
Determining Empirical Formula
« on: August 29, 2005, 11:34:27 AM »
I'm NOT looking for the answer...but clarification of the question...because as of now...I don't understand that the question means!

0.7549 g of a compound makes 1.9061g of CO2 and 0.3370g of H2O. Determine the empirical formula for this substance.

Does this mean that compound X (0.7548 g of it) is combusted and results in the CO2 and H2O. How would I find the empirical formula with this information? Can someone restate/clarify the question or point me in the right direction!!
Logged

Offline sdekivit

  • Chemist
  • Full Member
  • *
  • Posts: 403
  • Mole Snacks: +32/-3
  • Gender: Male
  • B.Sc Biomedical Sciences, Utrecht University
Re:Determining Empirical Formula
« Reply #1 on: August 29, 2005, 12:08:39 PM »
first calculate the amount of mols C in CO2. Then the amount of mols H in H2O then you know the molar ratio of a hydrocarbon compund.
Logged

Blueshawk

  • Guest
Re:Determining Empirical Formula
« Reply #2 on: August 29, 2005, 12:23:40 PM »
Quote from: kissoftalons on August 29, 2005, 11:34:27 AM
I'm NOT looking for the answer...but clarification of the question...because as of now...I don't understand that the question means!

0.7549 g of a compound makes 1.9061g of CO2 and 0.3370g of H2O. Determine the empirical formula for this substance.

Does this mean that compound X (0.7548 g of it) is combusted and results in the CO2 and H2O. How would I find the empirical formula with this information? Can someone restate/clarify the question or point me in the right direction!!

It appears to be a combustion problem.  Find the moles of each product..moles of CO2 and H2O.  Then do a comparison, ie  mole ratio.  You know that the starting material needs C and H.  So  CxHy + zO2.  Since you know the starting materials mass...This should help.
« Last Edit: August 29, 2005, 12:27:39 PM by Blueshawk »
Logged

Offline sdekivit

  • Chemist
  • Full Member
  • *
  • Posts: 403
  • Mole Snacks: +32/-3
  • Gender: Male
  • B.Sc Biomedical Sciences, Utrecht University
Re:Determining Empirical Formula
« Reply #3 on: August 29, 2005, 12:27:19 PM »
Quote from: Blueshawk on August 29, 2005, 12:23:40 PM
It appears to be a combustion problem.  Find the moles of each product..moles of CO2 and H2O.  Then do a comparison, ie  mole ratio.  You know that the starting material needs C, O, and H.  So  CxHyOz.  Since you know the starting materials mass...This should help.

Also a CxHy compund will result in CO2 and H2O.
Logged

Blueshawk

  • Guest
Re:Determining Empirical Formula
« Reply #4 on: August 29, 2005, 12:31:38 PM »
Quote from: sdekivit on August 29, 2005, 12:27:19 PM
Also a CxHy compund will result in CO2 and H2O.

Sdekivit...Sorry for the  typo...i meant to say CxHy and zO2, and not CxHyOz.  I had just modified it to read correctly.
Logged

Offline sdekivit

  • Chemist
  • Full Member
  • *
  • Posts: 403
  • Mole Snacks: +32/-3
  • Gender: Male
  • B.Sc Biomedical Sciences, Utrecht University
Re:Determining Empirical Formula
« Reply #5 on: August 29, 2005, 12:35:12 PM »
Quote from: Blueshawk on August 29, 2005, 12:31:38 PM
Sdekivit...Sorry for the  typo...i meant to say CxHy and zO2, and not CxHyOz.  I had just modified it to read correctly.

ok  :D
Logged
Pages: [1]   Go Up
« previous next »
Sponsored Links