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III. Formula Calculations (p. 226-233)

Ch. 3 & 7 – The Mole. III. Formula Calculations (p. 226-233). A. Percentage Composition. the percentage by mass of each element in a compound. 127.10 g Cu 159.17 g Cu 2 S. 32.07 g S 159.17 g Cu 2 S. A. Percentage Composition. Find the % composition of Cu 2 S.  100 =. %Cu =.

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III. Formula Calculations (p. 226-233)

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  1. Ch. 3 & 7 – The Mole III. Formula Calculations(p. 226-233) C. Johannesson

  2. A. Percentage Composition • the percentage by mass of each element in a compound C. Johannesson

  3. 127.10 g Cu 159.17 g Cu2S 32.07 g S 159.17 g Cu2S A. Percentage Composition • Find the % composition of Cu2S.  100 = %Cu = 79.852% Cu %S =  100 = 20.15% S C. Johannesson

  4. 28 g 36 g 8.0 g 36 g A. Percentage Composition • Find the percentage composition of a sample that is 28 g Fe and 8.0 g O.  100 = 78% Fe %Fe =  100 = 22% O %O = C. Johannesson

  5. A. Percentage Composition • How many grams of copper are in a 38.0-gram sample of Cu2S? Cu2S is 79.852% Cu (38.0 g Cu2S)(0.79852) = 30.3 g Cu C. Johannesson

  6. 36.04 g 147.02 g A. Percentage Composition • Find the mass percentage of water in calcium chloride dihydrate, CaCl2•2H2O? 24.51% H2O %H2O =  100 = C. Johannesson

  7. CH3 B. Empirical Formula • Smallest whole number ratio of atoms in a compound C2H6 reduce subscripts C. Johannesson

  8. B. Empirical Formula 1. Find mass (or %) of each element. 2. Find moles of each element. 3. Divide moles by the smallest # to find subscripts. 4. When necessary, multiply subscripts by 2, 3, or 4 to get whole #’s. C. Johannesson

  9. 1.85 mol 1.85 mol B. Empirical Formula • Find the empirical formula for a sample of 25.9% N and 74.1% O. 25.9 g 1 mol 14.01 g = 1.85 mol N = 1 N 74.1 g 1 mol 16.00 g = 4.63 mol O = 2.5 O C. Johannesson

  10. N2O5 B. Empirical Formula N1O2.5 Need to make the subscripts whole numbers  multiply by 2 C. Johannesson

  11. C2H6 C. Molecular Formula • “True Formula” - the actual number of atoms in a compound CH3 empirical formula ? molecular formula C. Johannesson

  12. C. Molecular Formula 1. Find the empirical formula. 2. Find the empirical formula mass. 3. Divide the molecular mass by the empirical mass. 4. Multiply each subscript by the answer from step 3. C. Johannesson

  13. 28.1 g/mol 14.03 g/mol C. Molecular Formula • The empirical formula for ethylene is CH2. Find the molecular formula if the molecular mass is 28.1 g/mol? empirical mass = 14.03 g/mol = 2.00 (CH2)2  C2H4 C. Johannesson

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