1 / 8

BRADY PROBLEM 2.83

BRADY PROBLEM 2.83. Tutorial on the procedure of solving for empirical and molecular formulas from a combustion reaction. H 2 O 0.1874 g. CO 2 0.6871 g. O 2. (C + H + O) 0.5000 g. +. +. Problem.

tori
Télécharger la présentation

BRADY PROBLEM 2.83

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. BRADY PROBLEM 2.83 Tutorial on the procedure of solving for empirical and molecular formulas from a combustion reaction.

  2. H2O0.1874 g CO20.6871 g O2 (C + H + O)0.5000 g + + Problem Citric Acid, the substance that makes lemon juice sour, is composed of only carbon , hydrogen, and oxygen. When a 0.5000 g sample of citric acid was burned, it produced 0.6871 g CO2 and 0.1874 g H2O. The molecular mass of the compound is 192. What are the empirical and molecular formulas for citric acid?

  3. H2O0.1874 g CO20.6871 g O2 (C + H + O)0.5000 g + + All the hydrogen has gone to theproduct ofH2O All the carbon has gone to the product of CO2 From these gram quantities, convert to moles of compound, then to moles of elements…(you may wish to subtotal as you will use the number of moles later)…then to grams of elements. Starting with CO2….

  4. Convert grams of CO2 to moles of CO2to moles of C then to grams of carbon.

  5. Convert grams of H2Oto moles of H2Oto moles of H then to grams of hydrogen.

  6. Find the number of grams of oxygenin the original sample Convert these grams to moles of oxygen

  7. Find the lowest mole ratio for the empirical formula C6H8O7

  8. C = 12.011 X 6 = 72.061H = 1.008 x 8 = 8.064O = 15.9994 x 7 = 111.99 192.12 g/mol Find the Molecular Formulafrom the given Molecular Weight Given molecular weight = 192 g/mol Empirical Formula determined: C6H7O7 Calculate the mass of the empirical formula: Divide the mass of the empirical into the molecular weight: 192/192.12 = 0.99938 = 1 therefore the empirical formula is the same as the molecular formula

More Related