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Section 9-2: Ideal Stoichiometric Calculations

Section 9-2: Ideal Stoichiometric Calculations. Coach Kelsoe Chemistry Pages 304–311. Section 9-2 Objectives. Calculate the amount in moles of a reactant or product from the amount in moles of a different reactant or product.

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Section 9-2: Ideal Stoichiometric Calculations

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  1. Section 9-2:Ideal Stoichiometric Calculations Coach Kelsoe Chemistry Pages 304–311

  2. Section 9-2 Objectives • Calculate the amount in moles of a reactant or product from the amount in moles of a different reactant or product. • Calculate the mass of a reactant or product from the amount in moles of a different reactant or product. • Calculate the amount in moles of a reactant or product from the mass of a different reactant or product. • Calculate the mass of a reactant or product from the mass of a different reactant or product.

  3. Ideal Stoichiometric Calculations • The chemical equation plays a very important part in all stoichiometric calculations because the mole ratio is obtained directly from it. Solving any reaction-stoichiometry problem must begin with a balanced equation. • Chemical equations help us make predictions about chemical reactions without having to run the reactions in the laboratory. • The calculations we make in this section are THEORETICAL. They tell us the amounts of reactants and products under ideal conditions.

  4. Ideal Stoichiometric Calculations • Ideal conditions are rarely met in the lab or in industry. Yet, theoretical stoichiometric calculations serve the very important function of showing the maximum amount of product that could be obtained before a reaction is run in the laboratory. • Solving stoichiometric problems requires practice. Use a logical and systematic approach along with your previous knowledge of chemistry to work through these problems.

  5. Conversions of Quantities in Moles • In these stoichiometric problems, you are asked to calculate the amount in moles of one substance that will react with or be produced from the given amount in moles of another substance. • The plan for a simple mole conversion problem is:Amount of Amount ofgivenunknownsubstance (in mol) substance (in mol)

  6. Conversions of Quantities in Moles • These type of problems require only one conversion factor: the mole ratio of the unknown substance to the given substance from the balanced equation. • given quantity x conversion factor = unknown quantity

  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 chemical equation: CO2(g) + 2LiOH(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. Sample Problem 9-1 • Given: amount of CO2 = 20 mol; formula- CO2(g) + 2LiOH(s)  Li2CO3(s) + H2O(l) • Unknown: amount of LiOH in moles • Answer:20 mol CO2 x 2 mol LiOH = 40 mol LiOH 1 mol CO2

  9. Sample Problem • 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? • Given: moles of hydrogen gas, H2,= 6 mol • Unknown: moles of ammonia, formula

  10. Sample Answer • N2 + H2 NH3 (unbalanced) • N2 + 3H2 2NH3 (balanced) • 6.0 mol H2 x 2 mol NH3 = 4.0 mol NH3 3 mol H2

  11. Conversions of Amounts in Moles to Mass • In the following calculations, you will be asked to calculate the mass of a substance that will react with or be produced from a given amount in moles of a second substance. • This plan requires two conversion factors: mole ratio of the unknown and given substances and the molar mass of the unknown substance.

  12. Conversions of Amounts in Moles to Mass • Amount of Amount of Mass ofgivenunknownunknownsubstance substance substance(in mol) (in mol) (in grams)

  13. 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? • Given: moles of water, H2O, = 3.00 mol • Unknown: balanced chemical equation, mass of glucose

  14. Sample Problem 9-2 • CO2 + H2O  C6H12O6 + O2 (unbalanced) • 6CO2 + 6H2O  C6H12O6 + 6O2 (balanced) • 3.00 mol H2O x 1 mol C6H12O6 x 180.18 g C6H12O6 = 90.1 g 6 mol H2O 6 mol C6H12O6

  15. Sample Problem • What mass of carbon dioxide, in grams, is needed to react with 3.00 mol of H2O in the photosynthetic reaction described in the last problem? • Given: moles of water, H2O, = 3.00 mol • Unknown: balanced chemical equation, mass of carbon dioxide

  16. Sample Problem • CO2 + H2O  C6H12O6 + O2 (unbalanced) • 6CO2 + 6H2O  C6H12O6 + 6O2 (balanced) • 3.00 mol H2O x 6 mol CO2 x 44.01 g CO2 = 132 g 6 mol H2O 1 mol CO2

  17. Conversions of Mass to Amounts in Moles • In these problems, you start with a mass and converting that mass to moles, then using another conversion factor to convert from your given substance to your unknown substance. • Mass of Amount of Amount ofgivengivenunknownsubstance substance substance(in grams) (in mol) (in mol)

  18. Sample Problem 9-3 • The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia. NH3(g) + O2(g)  NO(g) + H2O(g)The reaction is run using 824 g of NH3 and excess oxygen. How many moles of H2O are formed? • Given: mass of ammonia, NH3 = 824 g • Unknown: balanced chemical equation, moles of H2O

  19. Sample Problem 9-3 • NH3 + O2 NO + H2O (unbalanced) • 4NH3 + 5O2 4NO + 6H2O (balanced) • 824 g NH3 x 1 mol NH3 x 6 mol H2O = 72.6 mol 17.04 g NH3 4 mol NH3

  20. Mass-Mass Calculations • Mass-mass calculations are more practical than other mole calculations we’ve studied. • You can never measure moles directly. You are generally required to calculate the amount in moles of a substance from its mass, which you can measure in the lab. • Mass-mass problems can be viewed as the combination of the other types of problems.

  21. Mass-Mass Calculations • Mass of Amount of Amount of Mass ofgiven given unknown unknownsubstance substance substance substance(in grams) (in mol) (in mol) (in grams)

  22. Sample Problem 9-4 • 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) + 2HF  SnF2(s) + H2(g)How many grams of SnF2 are produced from the reaction of 30.00 g of HF with Sn? • Given: mass of HF, balanced equation • Unknown: mass of SnF2

  23. Sample Problem 9-4 • Step 1: Convert grams of given to moles of given. • Step 2: Convert moles of given to moles of unknown. • Step 3: Convert moles of unknown to grams of unknown. • 30.00 g HF x 1 mol HF x 1 mol SnF2 x 156.71 g SnF2 = 117.5 g 20.01 g HF 2 mol HF 1 mol SnF2

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