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For more information, please see full course syllabus of Chemistry
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Lecture Comments (7)

1 answer

Last reply by: Zachary McCoy
Fri Jan 3, 2014 10:54 PM

Post by Norman Cervantes on January 13, 2013

the squeaking of the pen is extremely distracting.

2 answers

Last reply by: Jamal Tischler
Wed Mar 18, 2015 1:57 PM

Post by alain simplice on October 6, 2012

why not show us how he get those number from periodic table?

1 answer

Last reply by: Jamal Tischler
Wed Mar 18, 2015 2:00 PM

Post by Atreya Mohile on May 5, 2012

Sir, I have a doubt in a question:
0.152 gram organic substance on combustion gives 0.304 gram of co2(carbon-dioxide) and 0.124 gram of h2o (water).The vapour density of substance is 44. Calculate the empirical formula and molecular formula of that substance. (H=1 , C=12 , O=16).

Empirical and Molecular Formulas

  • Learn how to calculate mass % of each element from molecular formula

  • Learn distinction between empirical and molecular formulas

  • Master calculation of empirical formulas from mass % of each element

  • Methods for determining molar mass include mass spectra; gas laws; and colligative properties of solutions

  • Learn how to go from empirical to molecular formulas; molecular = empirical x n where n is integer

Empirical and Molecular Formulas

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

  • Intro 0:00
    • Empirical Formula
    • Molecular Formula
  • Percentage by Mass 1:40
    • Elements in Compounds
    • Example: Water
    • Example: Copper Sulfate
  • Empirical Formula 13:02
    • Example: Hydrocarbons
  • Calculating Empirical Formula 20:24
    • Example: C, H, O
  • Molar Mass and Molecular Formulas 27:54
  • Determining Molar Mass 32:21
    • Mass Spectrometry
    • Gas Laws
    • Colligative Properties
  • Empirical and Molecular Formulas 39:30
    • Example: Ethylene and Chlorine
  • Additional Example 1
  • Additional Example 2