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EMPIRICAL FORMULA

EMPIRICAL FORMULA. The empirical formula represents the smallest ratio of atoms present in a compound. The molecular formula gives the total number of atoms of each element present in one molecule of a compound.

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EMPIRICAL FORMULA

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  1. EMPIRICAL FORMULA • The empirical formula represents the smallest ratio of atoms present in a compound. • The molecular formula gives the total number of atoms of each element present in one molecule of a compound. The empirical formula is the simplest formula and the molecular formula is the “true” formula.

  2. EMPIRICAL FORMULA Assume 100g sample Calculate mole ratio Use Atomic Masses Mass % of elements Empirical Formula Grams of each element Moles of each element

  3. EMPIRICAL FORMULA Step 1: If given the % composition, assume a 100g sample then convert % to grams. Step 2: Use the atomic masses to convert grams to moles. Step 3: Divide the moles of each element by the SMALLEST mole fraction. Step 4: The results from step 3 should be a whole number, if not, make it so by multiplying by a common factor.

  4. EMPIRICAL FORMULA 1. Calculate the empirical formula from a sample containing 43.4% Na, 11.3% C, and 45.3% O. smallest 43.4%  43.4 g Na (1 mole / 23 g/mol) =1.887 moles Na 11.3%  11.3 g C (1 mole / 12 g/mol) = 0.9417 moles C 45.3%  45.3 g O (1 mole / 16 g/mol) = 2.831 moles O 1.887/0.9417 =2.00 Na 2.831/0.9417 = 3.00 O . 9417/.9417 = 1.00 C Empirical Formula = Na2CO3

  5. EMPIRICAL FORMULA 2. When 8.00 g of calcium metal is heated in air, 11.20 g of metal oxide is formed. Calculate the empirical formula. According to the Law of Conservation of mass, 11.20 g Product - 8.00 g Ca = 3.20 g Oxygen (reactive part of air) smallest 8.00 g Ca (1 mole / 40 g/mol) = 0.200 moles Ca 3.20 g O (1 mole / 16 g/mol) = 0.200 moles O 0.200 / 0.200 = 1 Empirical Formula = CaO

  6. EMPIRICAL FORMULA 3. A compound was found to have a composition of 33.0 % Sr, 26.8 % Cl, and 40.2 % water. Calculate the empirical formula of this hydrate. smallest 33.0%  33.0 g Sr (1 mole/87.6 g/mol) = 0.3767 moles Sr 26.8%  26.8 g Cl (1 mole/35.45 g/mol) = 0.7560 moles Cl 40.2%  40.2 g H2O (1 mole/18.0g/mol) = 2.233 moles H2O 0.7560 / 0.3767 = 2 Cl 2.233 / 0.3767 = 5.9 = 6 H2O Empirical Formula = SrCl2 . 6 H2O

  7. EMPIRICAL FORMULA & Molecular Formula 4. Propylene contains 14.3 % H, 85.7% C, and has a molar mass of 42.0 g/mol. What is its molecular formula? smallest 14.3%  14.3 g H (1 mole/1.01 g/mol) = 14.19 moles H 85.7%  85.7 g C (1 mole/12.01 g/mol) = 7.142 moles C 14.19 / 7.142 = 1.987 = 2 H Empirical Formula = CH2 Molar mass / empirical mass = multipier (42.0 g/mol / 14.0 g/mol) = 3 3 x CH2 becomes the molecular formula C3H6

  8. PRACTICE PROBLEM #12 A ______ 1. Which contains the larger number of MOLES of atoms? a) 125.0 g KCl b) 25.0 g CaSO4 c) 17.0 g of N2 ______ 2. What is the empirical formula of the compound whose composition is 39.7% K, 27.8% Mn, and 32.5% O? ______ 3. Determine the empirical formula of a compound that contains 89.7 % bismuth and 10.3 % oxygen. ______ 4. Write the molecular formula for a compound that contains 54.5 % C, 9.1% H, and 36.4 % O and has a molar mass of 132 amu? K2MnO4 Bi2O3 C6H12O3

  9. GROUP STUDY PROBLEM #12 ______ 1. Which contains the larger number of MOLES of atoms? a) 125.0 g HBr b) 25.0 g C6H11O6 c) 17.0 g of Br2 ______ 2. A sample of a compound weighing 4.18 g contains 1.67 g of sulfur and the rest is oxygen. What is the empirical formula? ______ 3. What is the empirical formula of the compound whose composition is 28.7% K, 1.4% H, 22.8 % P, and 47.1% O? ______ 4. A compound contains 92.3% C and 7.7% H and has a molar mass of 78.0 g/mol. Determine the molecular formula.

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