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EMPIRICAL FORMULA empirical formulaThe empirical formula represents the smallest ratio of atoms present in a compound. molecular formulaThe molecular formula.

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Presentation on theme: "EMPIRICAL FORMULA empirical formulaThe empirical formula represents the smallest ratio of atoms present in a compound. molecular formulaThe molecular formula."— Presentation transcript:

1 EMPIRICAL FORMULA empirical formulaThe empirical formula represents the smallest ratio of atoms present in a compound. molecular formulaThe 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 Grams of eachelement Moles of eachelement EmpiricalFormula

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 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) = moles C 45.3%  45.3 g O (1 mole / 16 g/mol) = moles O 1.887/ =2.00 Na 2.831/ = 3.00 O. 9417/.9417 = 1.00 C Empirical Formula = Na 2 CO 3

5 EMPIRICAL FORMULA. 2. When 8.00 g of calcium metal is heated in air, g of metal oxide is formed. Calculate the empirical formula. According to the Law of Conservation of mass, g Product g Ca = 3.20 g Oxygen (reactive part of air) smallest smallest 8.00 g Ca (1 mole / 40 g/mol) = moles Ca 3.20 g O (1 mole / 16 g/mol) = moles O / = 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 smallest 33.0%  33.0 g Sr (1 mole/87.6 g/mol) = moles Sr 26.8%  26.8 g Cl (1 mole/35.45 g/mol) = moles Cl 40.2%  40.2 g H 2 O (1 mole/18.0g/mol) = moles H 2 O / = 2 Cl / = 5.9 = 6 H 2 O Empirical Formula = SrCl 2. 6 H 2 O

7 EMPIRICAL FORMULA & Molecular Formula 4. smallest 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) = moles H 85.7%  85.7 g C (1 mole/12.01 g/mol) = moles C / = = 2 H Empirical Formula = CH 2 Molar mass / empirical mass = multipier (42.0 g/mol / 14.0 g/mol) = 3 3 x CH 2 becomes the molecular formula  C 3 H 6

8 PRACTICE PROBLEM #12 ______ 1. Which contains the larger number of MOLES of atoms? a) g KCl b) 25.0 g CaSO 4 c) 17.0 g of N 2 ______ 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? A K 2 MnO 4 Bi 2 O 3 C 6 H 12 O 3

9 GROUP STUDY PROBLEM #12 ______ 1. Which contains the larger number of MOLES of atoms? a) g HBr b) 25.0 g C 6 H 11 O 6 c) 17.0 g of Br 2 ______ 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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