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Civil Rights Act Signed into Law ( 1964)

Civil Rights Act Signed into Law ( 1964). HW 8: DUE Monday 7/7/14 ( only assignment from this chapter) Chap. 8, #'s 5, 11, 19-27 odd, 33, 35, 37, 39,55-61 odd, 77, 79, 81, 85, 92, 117, 121, 122, 123 Lab Tomorrow (WET LAB!) No prelab Exam 2 on Thursday

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Civil Rights Act Signed into Law ( 1964)

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  1. Civil Rights Act Signed into Law (1964) • HW8: DUE Monday7/7/14(only assignment from this chapter) • Chap. 8, #'s 5, 11, 19-27 odd, 33, 35, 37, 39,55-61 odd, 77, 79, 81, 85, 92, 117, 121, 122, 123 • Lab Tomorrow (WET LAB!) • No prelab • Exam 2 on Thursday • Monday - Nomenclature Proficiency Quiz 1 • Wednesday – DA/Math Proficiency Quiz 2

  2. Empirical Formulae The simplest whole number ratio of atoms in a molecule Example: molecular formula = C6H12O2 empirical formula = C3H6O Example: molecular formula = C16H32O2N4 empirical formula = C8H16ON2 Example: molecular formula = KMnO4 empirical formula = KMnO4

  3. Calculating Empirical Formulae What is the empirical formula of a compound that is made up of 10.95g C, 29.25g O, and 34.75g F? Step 1: convert each mass to MOLES Step 2: divide EACH by the smallest!!

  4. Calculating Empirical Formulae What is the empirical formula of a compound that is made up of 10.95g C, 29.25g O, and 34.75g F? So we have 1 mol C, 2 mol O, and 2 mol F Step 3: if each is a whole number, write the empirical formula CO2F2

  5. Calculating Empirical Formulae What is the empirical formula of a compound that is made up of 32.79% Na, 13.02% Al, and 54.19% F? Step 1: assume 100 g THEN convert each mass to MOLES Step 2: divide EACH by the smallest!!

  6. Calculating Empirical Formulae What is the empirical formula of a compound that is made up of 32.79% Na, 13.02% Al, and 54.19% F? So we have 3 mol Na, 1 mol Al, and 6 mol F Step 3: if each is a whole number, write the empirical formula Na3AlF6

  7. Calculating Empirical Formulae What is the empirical formula of a compound that is made up of 62.1% C, 5.21% H, 12.1% N, and 20.7% O? Step 1: assume 100 g THEN convert each mass to MOLES Step 2: divide EACH by the smallest!!

  8. Calculating Empirical Formulae What is the empirical formula of a compound that is made up of 62.1% C, 5.21% H, 12.1% N, and 20.7% O? So we have 6 mol C, 6 mol H, 1 mol N, and 1.5 mol O Step 3: if each is a whole number, write the empirical formula Step 3a: multiply EACH ELEMENT by the smallest number that will make all of them whole numbers C6H6NO1.5 O 1.5 x 2 = 3 C 6 x 2 = 12 H 6 x 2 = 12 N 1 x 2 = 2 C12H12N2O3

  9. What is the empirical formula of a compound made up of 74.01% C, 5.23% H, and 20.76% O? Step 1: assume 100 g THEN convert each mass to MOLES Step 2: divide EACH by the smallest!!

  10. What is the empirical formula of a compound made up of 74.01% C, 5.23% H, and 20.76% O? So we have 4.75 mol C, 4 mol H, and 1 mol O Step 3: If all of the subscripts are NOT whole numbers, then multiply EACH ELEMENT by the smallest number that will make all of them whole numbers C4.75H4O C19H16O4 multiply EACH of the subscripts by 4! H 4 x 4 = 16 O 1 x 4 = 4 C 4.75 x 4 = 19

  11. Molecular Formulae: The Next Step What is the empirical formula of: C6H9N3 ratio = 3 to 1 C2H3N What are the molar masses of the molecular and empirical formulae? C6H9N3 = 123.18 g/mol ratio = 3 to 1 C2H3N = 41.06 g/mol

  12. Molecular Formulae: The Next Step Molecular formula and empirical formula will always have the same ratio as the molecular mass and the empirical mass! If a compound has a molar mass of 78.1150 g/mol and an empirical formula of CH, what is the molecular formula? empirical mass = 13.02 g/mol mass ratio = 6 to 1 6(CH)  C6H6 formula ratio = 6 to 1 molecular formula = C6H6

  13. Molecular Formulae: The Next Step Caffeine is my life blood! Give the empirical and molecular formulae based on: 40.09g C, 4.172g H, 23.41g N, and 13.37g O. The molar mass of caffeine is 194.19 g/mol C4H5N2O

  14. Molecular Formulae: The Next Step Caffeine is my life blood! Give the empirical and molecular formulae based on: 40.09g C, 4.172g H, 23.41g N, and 13.37g O. The molar mass of caffeine is 194.19 g/mol C4H5N2O C4H5N2O = 97.11 g/mol mass ratio = 2 to 1 2(C4H5N2O)  C8H10N4O2 formula ratio = 2 to 1 molecular formula = C8H10N4O2

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