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Section 9.2 Ideal Stoichiometric Calculations

Section 9.2 Ideal Stoichiometric Calculations. Objectives. Basic Sentence: Calculate the______________ of a reactant or product from the ____________ of a different reactant or product. 1. amount in moles; amount in moles 2. mass; amount in moles

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Section 9.2 Ideal Stoichiometric Calculations

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  1. Section 9.2Ideal Stoichiometric Calculations

  2. Objectives • Basic Sentence: Calculate the______________ of a reactant or product from the ____________ of a different reactant or product. 1. amount in moles; amount in moles 2. mass; amount in moles 3. amount in moles; mass 4. mass; mass

  3. Solving Any Stoichiometry Problem • Must begin with a balanced equation. • For this chapter we assume that the amounts of reactants and products for a given reaction occur under ideal conditions.

  4. Ideal Conditions • All reactants are completely converted into products. • This rarely happens in the lab or in industry

  5. Yet… • Theoretical calculations are important because they show the maximum amount of product that could be obtained.

  6. Calculate the moles of a reactant or product from the moles of a different reactant or product. Conversions of Amounts in Moles to Moles mole given xmol unknown =mol unknown mol given Mole Ratio

  7. Sample Problem 9-1 In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following: CO2 (g) + 2 LiOH (s) → Li2CO3 (s) + H2O (l) How many moles of lithium hydroxide are required to react with 20 mol of CO2, the average amount exhaled by a person each day?

  8. Practice Problem #1 Ammonia, NH3, is widely used as a fertilizer and in many household cleaners. How many moles of ammonia are produced when 6 mol of hydrogen gas react with an excess of nitrogen gas?

  9. Practice Problem #2 The decomposition of potassium chlorate, KClO3, is used as a source of oxygen in the laboratory. How many moles of potassium chlorate are needed to produce 15 mol of oxygen?

  10. Conversions of Amounts in Moles to Mass Mole ratio Calculate thegramsof a reactant or product from the moles of a different reactant or product. Mol of unknown Grams of unknown Mol given Molar mass

  11. Sample Problem 9-2 In photosynthesis, plants use energy from the sun to produce glucose, C6H12O6 and oxygen from the reaction of carbon dioxide and water. What mass, in grams, of glucose is produced when 3.00 mol of water react with carbon dioxide?

  12. Sample Problem 9-3 What mass of carbon dioxide, in grams, is needed to react with 3.00 mol of H2O in the photosynthetic reaction described in Sample Problem 9-2?

  13. Practice Problem #1 When magnesium burns in air, it combines with oxygen to form magnesium oxide according to the following equation: 2 Mg (s) + O2 (g) → 2 MgO (s) What mass in grams of magnesium oxide is produced from 2.00 moles of magnesium?

  14. Practice Problem #2 What mass in grams of oxygen combines with 2.00 mol of magnesium in this same reaction?

  15. Practice Problem #3 What mass of glucose can be produced from a photosynthesis reaction that occurs using 10 mol CO2? 6 CO2(g)+6 H2O (l) → C6H12O6(aq) +6O2(g)

  16. Conversions of Mass to Amounts in Moles Calculate the moles of a reactant or product from the grams of a different reactant or product. Molar mass Mole ratio Mol of unknown Mass given Mol of given

  17. Sample Problem 9-4 The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia: NH3 (g) + O2 (g) → NO (g) + H2O (g) (unbalanced) The reaction is run using 824 g of NH3 and excess oxygen. How many moles of NO are formed? How many moles of H2O are formed?

  18. Practice Problem #1 and #2 Oxygen was discovered by Joseph Priestley in 1774 when he heated mercury (II) oxide to decompose it to form its constituent elements. How many moles of mercury (II) oxide, HgO, are needed to produce 125 g of oxygen, O2? How many moles of mercury are produced?

  19. Conversions of Mass to Mass Molar mass Mole ratio Mol of unknown Mass of given Mol of given Calculate thegramsof a reactant or product from the grams of a different reactant or product. Molar mass mass of unknown

  20. Sample Problem 9-5 Tin (II) fluoride, SnF2, is used in some toothpastes. It is made by the reaction of tin with hydrogen fluoride according to the following equation: Sn (s) + 2 HF (g) → SnF2 (s) + H2 (g) How many grams of SnF2 are produced from the reaction of 30.00g of HF with Sn?

  21. Laughing gas (nitrous oxide, N2O) is sometimes used as an anesthetic in dentistry. It is produced when ammonium nitrate is decomposed according to the following reaction: NH4NO3 (s) → N2O (g) + 2 H2O (l) a. How many grams of NH4NO3 are required to produce 33.0 g of N2O? b. How many grams of water are produced in this reaction?

  22. Practice Problem #2 When copper metal is added to silver nitrate in solution, silver metal and copper (II) nitrate are produced. What mass of silver is produced from 100. g of Cu?

  23. Practice Problem #3 What mass of aluminum is produced by the decomposition of 5.0 kg of Al2O3?

  24. Assignments – Due Tomorrow 9.2 Textbook Problems

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