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Molecular and empirical formulas

Molecular and empirical formulas. What’s in this stuff?. % composition. What does a % show us? % composition shows what ratios are in a compound Formula % comp = mass of element x 100 mass of compound What is the % composition of elements in Glucose

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Molecular and empirical formulas

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  1. Molecular and empirical formulas What’s in this stuff?

  2. % composition • What does a % show us? • % composition shows what ratios are in a compound • Formula • % comp = mass of element x 100 mass of compound • What is the % composition of elements in • Glucose • Sodium floride • Ammonium chloride

  3. Calculate an empirical formula • Empirical – capable of being confirmed by observation or experimentation • Empirical formula are based upon % composition • The empirical formula is the lowest ratio of elements in the compound • For ionic compounds the empirical formulas are usually the same as molecular formula • A compound has a % comp of 25.9 % nitrogen and 74.1% oxygen

  4. White board practice • 72.2% Mg 27.8 % nitrogen • Glucose contains 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass.

  5. Calculate molecular formula • Molecular formula is the formula on the bottle on the shelf, this is the actual chemical formula • Based upon the empirical formula • And the mass of the actual compound • Example A compound has an empirical formula of NO2 and a molar mass of 92.02 g/mol.

  6. practice • Ibuprofen, a common headache remedy, has an empirical formula of C7H9O and a molar mass of approximately 215 g/mol. • Nicotine is 74.1% carbon, 8.6% hydrogen, and 17.3% nitrogen by mass. Its molar mass is about 160 g/mol.

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