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Chapter 9

Stoichiometry. Chapter 9. I. STOICHIOMETRY. Describes the mass and mole relationships in a chemical reaction Use it to predict the amount of product formed or the amount of reactant needed in a particular reaction. EXAMPLES. How many moles of each product are formed:

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Chapter 9

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  1. Stoichiometry Chapter 9

  2. I. STOICHIOMETRY • Describes the mass and mole relationships in a chemical reaction • Use it to predict the amount of product formed or the amount of reactant needed in a particular reaction

  3. EXAMPLES • How many moles of each product are formed: Sodium Chloride  Sodium + Chlorine  + 2 NaCl 2 Na Cl2 2.0 moles 2.0 moles 1.0 moles 4.0 moles 4.0 moles 2.0 moles 1.0 moles 1.0 moles 0.5 moles 8.0 moles 8.0 moles 4.0 moles

  4. EXAMPLES • Sodium Chlorate  Sodium Chloride + Oxygen  + 2 NaClO3 2 NaCl 3 O2 4.0 moles 6.0 moles 4.0 moles .378 moles .378 moles .567 moles

  5. EXAMPLES 3. How many moles of Oxygen are produced from the decomposition of .849 moles of Potassium Chlorate? Potassium Chlorate  Potassium Chloride + Oxygen 2 KClO3  2 KCl + 3 O2

  6. EXAMPLES • How many grams of Water are produced from the decomposition of 1.42 moles of Sodium Hydroxide? Sodium Hydroxide  Sodium Oxide + Water 2 NaOH Na2O + H2O

  7. EXAMPLES • How many moles of Hydrogen are produced from the reaction of 2.10 moles of Sodium with Water? Sodium + Water  Sodium Hydroxide + Hydrogen 2 Na + H2O  NaOH + H2

  8. EXAMPLES • Determine the mass of Fluorine that must react with Lithium to produce 12.0 grams of Lithium Fluoride. Lithium + Fluorine  Lithium Fluoride 2 Li + F2 LiF 2

  9. II. LIMITING REACTANT • The reactant that is present in least abundance (less amount of moles) determines the amount of product formed. • Example: You need to make as many cakes as possible. Each cake requires 2 eggs, 2 cups of flour, and 1 cup of sugar. You have 6 eggs, 6 cups of sugar, and 4 cups of flour. Which is your limiting reactant (ingredient)?

  10. EXAMPLES • Circle the limiting reactant: NaHCO3 + HCl NaCl + H2O + CO2 Given: 1.0 mole 1.5 mole Actual: 1.0 mole 1.0 mole 1.0 mole 1.0 mole 1.0 mole Given: .475 mole .214 mole Actual: .214 mole .214 mole .214 mole .214 mole .214 mole

  11. Examples • Mg + 2 HCl MgCl2 + H2 Given: 1.0 mole 1.5 mole Actual: Given: 2.0 mole 4.5 mole Actual:

  12. Examples • 2 Al + 3 S  Al2S3 Given: 4.0 mole 5.0 mole Actual:

  13. Examples • If 1.00 gram of Hydrogen reacts with 6.00 grams of Oxygen, determine the mass of product formed.

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