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Ch 3 Friday

# Ch 3 Friday - Chapter 3 Chemical Equations Stoichiometry...

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1 Stoichiometry: Calculations with Chemical Formulas and Equations Chapter 3 Chapter 3 Chemical Equations Balancing, Types of Equations Compound Composition Atom mass; Atomic and formula weight % Composition Empirical Formulas/Molecular Formulas Mole ratio - Stoichiometry Amounts in chemical reactions Limiting reagents Theoretical yield Percent yield Determining the Empirical Formula Can we determine the formula for a compound from the % composition? Empirical formula % Composition (mole ratio) (mass ratio) Determining the Empirical Formula for a Compound Given that the % composition of a compound is 30.45% N and 69.56% O , what is the empirical formula for the compound? 1. Assume 100 g of compound 2. Convert g of each element to moles. 3. Divide or multiply each by the same number to get whole-number subscripts. Determining the Empirical Formula for a Compound Given that the % composition of a compound is 30.45% N and 69.56% O , what is the formula for the compound? 1. Assume 100 g of compound 30.45 g N 69.56 g O Determining the Empirical Formula for a Compound Given that the % composition of a compound is 30.45% N and 69.56% O , what is the formula for the compound? 2. Convert grams of each element to moles. (30.45 g N)(1 mol/14.01g N) = 2.173 mol N (69.56 g O)(1 mol/16.00g O) = 4.348 mol O

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