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Percent Composition and Chemical Formulas

Percent Composition and Chemical Formulas. Prentice-Hall Chapter 10.3 Dr. Yager. Objectives. Describe how to calculate the percent of mass of an element in a compound. Interpret an empirical formula. Distinguish between empirical and molecular formulas. Percent Composition of a Compound.

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Percent Composition and Chemical Formulas

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  1. Percent Composition and Chemical Formulas Prentice-Hall Chapter 10.3 Dr. Yager

  2. Objectives • Describe how to calculate the percent of mass of an element in a compound. • Interpret an empirical formula. • Distinguish between empirical and molecular formulas.

  3. Percent Composition of a Compound The percent by mass of an element in a compound is the number of grams of the element divided by the mass in grams of the compound, multiplied by 100%.

  4. Percent Composition from Mass Data The relative amounts of the elements in a compound are expressed as the percent composition or the percent by mass of each element in the compound.

  5. Percent Composition from the Chemical Formula

  6. Percent Composition as a Conversion Factor You can use percent composition to calculate the number of grams of any element in a specific mass of a compound.

  7. Propane (C3H8) is 81.8% carbon and 18% hydrogen. You can calculate the mass of carbon and the mass of hydrogen in an 82.0 g sample of C3H8.

  8. Ethyne (C2H2) is a gas used in welder’s torches. Styrene (C8H8) is used in making polystyrene. These two compounds of carbon have the same empirical formula (CH) but different molecular formulas.

  9. Empirical Formulas The empirical formula of a compound shows the smallest whole-number ratio of the atoms in a compound.

  10. Molecular Formula Compared to Empirical Formula The molecular formula of a compound is either the same as its experimentally determined empirical formula, or it is a simple whole-number multiple of its empirical formula.

  11. Methonal, ethanoic acid, and glucose all have the same empirical formula -CH2O.

  12. 1.Calculate the percent by mass of carbon in cadaverine, C5H14N2, a compound present in rotting meat. • 67.4% C • 58.8% C • 51.7% C • 68.2% C

  13. 1.Calculate the percent by mass of carbon in cadaverine, C5H14N2, a compound present in rotting meat. • 67.4% C • 58.8% C • 51.7% C • 68.2% C

  14. 2. Which of the following is NOT an empirical formula? • NO2 • H2N • CH • C3H6

  15. 2. Which of the following is NOT an empirical formula? • NO2 • H2N • CH • C3H6

  16. 3. Determine the molecular formula of a compound that contains 40.0 percent C, 6.71 percent H, and 53.29 percent O and has a molar mass of 60.05 g. • C2H4O2 • CH2O • C2H3O • C2H4O

  17. 3. Determine the molecular formula of a compound that contains 40.0 percent C, 6.71 percent H, and 53.29 percent O and has a molar mass of 60.05 g. • C2H4O2 • CH2O • C2H3O • C2H4O

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