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**Empirical and Molecular Formulas**

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**Empirical and Molecular Formulas**

An empirical formula shows the simplest whole number ratio of atoms of each element in a compound A molecular formula shows the actual number of atoms of each element in a compound

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**Example: Glucose Glucose has a molecular formula of:**

C6H12O6 It has an empirical formula of: CH2O

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Formulas cont’d A molecular formula is always a multiple of empirical formula A compound has ONE molecular formula Many compounds have the same empirical formula

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Example 0.18 grams of magnesium react with 0.12 grams of oxygen to form magnesium oxide Convert all grams to moles Divide all numbers of moles by the smallest # present (do a ratio!) Multiply all numbers by the smallest # that will make them WHOLE NUMBERS

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Example An oxide of aluminum is formed with g of Aluminum and g of Oxygen. Calculate the empirical formula of the compound: Convert all grams to moles Divide all numbers of moles by the smallest # present (do a ratio!) Multiply all numbers by the smallest # that will make them WHOLE NUMBERS

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**Find molecular formulas from empirical formulas**

A white powder is analyzed and found to have an empirical formula of P2O5. It has a molar mass of g/mol. What is the molecular formula for this compound?

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Section 12.2: Using Moles (part 3). Mass Percent Steps: 1) Calculate mass of each element 2) Calculate total mass 3) Divide mass of element/ mass of compound.

Section 12.2: Using Moles (part 3). Mass Percent Steps: 1) Calculate mass of each element 2) Calculate total mass 3) Divide mass of element/ mass of compound.

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