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Stoichiometry

Stoichiometry. It’s Finally Here!. What in the world is Stoichiometry?. Stoichiometry is how we figure out how the amounts of substances we need for a reaction or the amounts of substances produced in a reaction. We have to use the mole to mole relationship from the balanced equation.

marcellus-alston
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Stoichiometry

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  1. Stoichiometry It’s Finally Here!

  2. What in the world is Stoichiometry? • Stoichiometry is how we figure out how the amounts of substances we need for a reaction or the amounts of substances produced in a reaction We have to use the mole to mole relationship from the balanced equation

  3. Mole to Mole Relationship

  4. Example Problem • How many moles of silver can be produced by the reaction of 0.500mol of copper with silver nitrate if copper(II) nitrate is also produced?

  5. Example Problem • How many moles of oxygen are necessary to react with 0.450mol of iron to form iron(III) oxide?

  6. Example Problem • How many moles of carbon dioxide gas can be produced by the decomposition of 0.100mol of iron(III) carbonate?

  7. Practice Problem • How many moles of sodium phosphate are needed to completely react with 0.400mol copper(II) chloride?

  8. Practice Problem • How many moles of zinc are needed to completely react with 0.300mol hydrochloric acid?

  9. Practice Problem • How many moles of potassium chlorate are needed to generate 0.150mol oxygen gas?

  10. Mass-Mass Relationships

  11. Mass to Mass

  12. Example Problem • What mass of aluminum oxide can be produced by the reaction of 8.95g of aluminum with excess oxygen?

  13. Example Problem • What mass of water can be produced by the decomposition of 2.50g of iron(III) hydroxide?

  14. Example Problem • What mass of propane (C3H8) can be burned in 6.60g oxygen?

  15. Practice Problem • What mass of copper(II) oxide will remain after heating 5.50g copper(II) carbonate to decomposition?

  16. Practice Problem • What mass of oxygen is required to completely oxidize 4.50g of aluminum metal?

  17. Practice Problem • What mass of hydrogen can be produced by the reaction of 10.0g of sodium with water?

  18. Solution Volume Relationships

  19. Adding Volume

  20. Example Problem • What volume of 6.0M hydrochloric acid is required to completely react with 500.0mL of 0.0112M barium hydroxide?

  21. A Little Bit of Vocabulary • Titration – a method of chemical analysis used to determine the unknown concentration of a substance. This is done by reacting the substance with the unknown concentration with a substance of known concentration (a standard) and using the stoichiometric relationship from the reaction of the two substances to determine the unknown concentration.

  22. Example Problem • A 12.12mL portion of hydrochloric acid is used to titrate 0.512g of sodium hydrogen carbonate. What is the molarity of the hydrochloric acid solution?

  23. Example Problem • What volume of 0.105M NaOH is required to completely react with 1.00g of citric acid, H3C6H5O7?

  24. Example Problem • 10.0mL of 0.150M oxalic acid solution, H2C2O4 was titrated with 23.49mL of NaOH. What was the concentration of NaOH used in the titration??

  25. Gas Volume Relationships

  26. Gas Volumes • Gas volumes vary tremendously based on: • Pressure • Temperature • Amount of gas

  27. Gasses • To keep things simple: • Standard Pressure = 1 atmosphere (1 atm) • Standard Temperature = 0°C • STP = Standard Temperature and Pressure

  28. Example • What volume of oxygen gas is required to completely burn 1.0L of propane gas (C3H8) at STP?

  29. Example • What volume of oxygen gas can be produced at STP by the decomposition of 3.00g of potassium chlorate?

  30. Practice • What mass of sodium hydroxide is needed to completely react with 2.00L of carbon dioxide if sodium hydrogen carbonate is formed?

  31. Practice • What volume of hydrogen gas is produced when 22.5mL of 1.50M hydrochloric acid reacts with excess calcium?

  32. Limiting Reagent Practice

  33. Practice • 2.00g of magnesium ribbon is added to a 4.0L container of oxygen at STP. How many grams of magnesium oxide can be produced?

  34. Practice • A 1.25g piece of aluminum was added to 50.0mL of 0.100M copper(II) nitrate solution. How many grams of copper can be produced?

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