1. Stoichiometry It’s Finally Here!

3. 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

4. Mole to Mole Relationship

5. 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? 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?

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

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

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

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

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

11. Mass-Mass Relationships

12. Mass to Mass

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

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

15. Example Problem What mass of propane (C 3 H 8 ) can be burned in 6.60g oxygen? What mass of propane (C 3 H 8 ) can be burned in 6.60g oxygen?

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

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

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

19. Solution Volume Relationships

20. Adding Volume

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

22. 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.

23. 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? 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?

24. Example Problem What volume of 0.105M NaOH is required to completely react with 1.00g of citric acid, H 3 C 6 H 5 O 7 ? What volume of 0.105M NaOH is required to completely react with 1.00g of citric acid, H 3 C 6 H 5 O 7 ?

25. Example Problem 10.0mL of 0.150M oxalic acid solution, H 2 C 2 O 4 was titrated with 23.49mL of NaOH. What was the concentration of NaOH used in the titration?? 10.0mL of 0.150M oxalic acid solution, H 2 C 2 O 4 was titrated with 23.49mL of NaOH. What was the concentration of NaOH used in the titration??

26. Gas Volume Relationships

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

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

30. Example What volume of oxygen gas is required to completely burn 1.0L of propane gas (C 3 H 8 ) at STP? What volume of oxygen gas is required to completely burn 1.0L of propane gas (C 3 H 8 ) at STP?

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

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

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

34. Limiting Reagent Practice

35. 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? 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?

36. 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? 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?