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Unit: Chemical Quantities

Learn how to determine the empirical formulas of compounds using their percent makeup. Follow step-by-step instructions to convert percent composition to grams, then convert to moles and divide by the smallest mole value to obtain the empirical formula. Practice with examples provided.

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Unit: Chemical Quantities

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  1. Day 6 - Notes Unit: Chemical Quantities Determining the Empirical Formula from Percent Composition

  2. After today, you will be able to… Calculate the empirical formulas for various compounds given their percent makeup

  3. Empirical Formula Determination from % Composition To determine empirical formulas from % composition follow these steps: • Assume 100.0g of the compound (change % into grams) • Convert g moles for each element using molar mass • Divide each mole answer by the smallest mole answer • If you do not have a whole number, multiply by the smallest whole # to get a whole # ratio. • Skip to this step if you already have a whole number ratio from #3. These whole #s are the subscripts for each element.

  4. To sum up these steps here is a poem for my favorite little chemists: “Percent to mass Mass to Moles Divide by small Multiply by whole!”

  5. Example: What is the empirical formula for a compound that is 21.2% N, 6.10% H, 24.3% S, and 48.4%O? 1 mol N 14.01gN 1.51 21.2gN 6.10gH 24.3gS 48.4gO x = = 2 0.758 0.758 0.758 0.758 1 mol H 1.01gH 6.04 = x 7.97~ = 8 N2H8SO4 1 mol S 32.07gS 0.758 = x = 1 3.03 1 mol O 16.00gO = x = 4

  6. Example: What is the empirical formula for a compound that is 69.8% Fe and 30.2% O? 1 mol Fe 55.85gFe 1.25 69.8gFe 30.92gO x = = 1 (2) = 2 1.25 1.25 1.89 1 mol O 16.00gO (2) 1.5 3 = x = = Fe2O3

  7. HOMEWORK: Time to Practice!Complete WS 6

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