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the Mole !

It’s time to learn about. the Mole !. What's The Difference Between Roast Beef And Pea Soup?. Anyone Can Roast Beef. Stoichiometry. Stoichiometry : Mole Ratios to Determining Grams of Product At the conclusion of our time together, you should be able to:.

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the Mole !

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  1. It’s time to learn about . . . the Mole !

  2. What's The Difference Between Roast Beef And Pea Soup? Anyone Can Roast Beef.

  3. Stoichiometry

  4. Stoichiometry : Mole Ratios to Determining Grams of ProductAt the conclusion of our time together, you should be able to: • Review the conversion of particles or grams to moles • Determine mole ratios from a balanced chemical equation • Determine the amount of product produced when given the amount of reactants

  5. Review the Molar Mass of Compounds • The molar mass (MM) of a compound is determined by adding up all the atomic masses for the molecule (or compound) • Ex. Molar mass of CaCl2 • Avg. Atomic mass of Calcium = 40.08g • Avg. Atomic mass of Chlorine = 35.45g • Molar Mass of calcium chloride = 40.08 g/mol Ca + (2 X 35.45) g/mol Cl 110.98 g/mol CaCl2 20 Ca40.08 17Cl 35.45

  6. Practice • Calculate the Molar Mass of calcium phosphate • Formula = • Masses elements: • Molar Mass = 310.18 g Ca3(PO4)2

  7. My new book on GOLF will give the reader valuable playing tips and insider information I've gained through my years of lessons, struggles and experiments. Here are just a few of the chapter titles:  Chapter 5 - When to Give the Ranger the Middle Digit. Chapter 14 – The Best Time to Let a Foursome Play through Your Twosome.

  8. Calculations molar mass Avogadro’s number Grams Moles Particles Everything must go through Moles!!!

  9. Flowchart Atoms or Molecules Divide by 6.02 X 1023 Multiply by 6.02 X 1023 Multiply by atomic/molar mass from periodic table Moles Divide by atomic/molar mass from periodic table Mass (grams)

  10. Chocolate Chip Cookies!! 1 cup butter 2 eggs 1/2 cup white sugar 1 teaspoon salt 1 cup packed brown sugar 1 teaspoon vanilla extract 2 1/2 cups all-purpose flour 1 teaspoon baking soda 2 cups semisweet chocolate chips Makes 3 dozen How many eggs are needed to make 3 dozen cookies? How much butter is needed for the amount of chocolate chips used? How much brown sugar would I need if I had 1½ cups white sugar?

  11. Cookies and Chemistry…Huh!?!? • Just like chocolate chip cookies have recipes, chemists have recipes as well • Instead of calling them recipes, we call them chemical equations • Furthermore, instead of using cups and teaspoons, we use moles • Lastly, instead of eggs, butter, sugar, etc. we use chemical compounds as ingredients

  12. Chemistry Recipes • Looking at a reaction tells us how much of something you need to react with something else to get a product (like the cookie recipe) • Be sure you have a balanced reaction before you start! Balance #1 on your worksheet!! • Example: 2 Ag+ Cl2  2 AgCl • This reaction tells us that by mixing 2 moles of silver with 1 mole of chlorine we will get 2 moles of silver chloride • What if we wanted 4 moles of AgCl? • 10 moles? • 50 moles?

  13. Let’s sit down and figure this out!!

  14. Practice • Write the balanced reaction for hydrogen gas reacting with oxygen gas. 2 H2 + O2 2 H2O • How many moles of reactants are needed? • What if we wanted 4 moles of water? • What if we had 3 moles of oxygen, how much hydrogen would we need to react, and how much water would we get? • What if we had 50 moles of hydrogen, how much oxygen would we need, and how much water would be produced?

  15. Mole Ratios • These mole ratios can be used to calculate the moles of one chemical from the given amount of a different chemical • Example: How many moles of chlorine are needed to react with 5 moles of silver (without any silver left over)? 2 Ag + Cl2 2 AgCl 5 Ag + 2.5 Cl2 5 AgCl

  16. x 1 mol Cl2 2 mol Ag Question Answer 2 Ag+ Cl2 2 AgCl # moles of Cl2 = 5 mol Ag = 2.5 mol Cl2

  17. 2 mol AgCl 1 mol Cl2 Mole-Mole Conversions • How many moles of silver chloride will be produced if you react 2.6 moles of chlorine gas with an excess (more than you need) of silver metal? 2 Ag + Cl2 2 AgCl # moles of AgCl = 2.6 mol Cl2 x = 5.2 mol AgCl

  18. Mass-Mole • We can also start with mass and convert to moles of product or another reactant • We use molar mass and the mole ratio to get to moles of the compound of interest • Calculate the number of moles of the combustion of ethane (C2H6) needed to produce 10.0 g of water • 2 C2H6 + 7 O2 4 CO2 + 6 H20

  19. x 2 mol C2H6 6 mol H2O x 1 mol H2O 18.02 g H2O Mass-Mole • 2 C2H6 + 7 O2 4 CO2 + 6 H20 10.0 g H2O = 0.185 mol C2H6

  20. A Comparison of the Arousal of the Sexes

  21. Start your HomeLearning NOW!!

  22. Stoichiometry Continued:

  23. Stoichiometry : Mole Ratios to Determining Grams of ProductAt the conclusion of our time together, you should be able to: • Review the conversion of particles or grams to moles • Determine mole ratios from a balanced chemical equation • Determine the amount of product produced when given the amount of reactants

  24. Mass-Mass Conversions • Most often we are given a starting mass and want to find out the mass of a product we will get (called theoretical yield) or how much of another reactant we need to completely react with it (no leftover ingredients!) • Now we must go from grams to moles, to mole ratios, and back to grams of the compound we are interested in.

  25. Mass-Mass Conversion • Ex. Calculate how many grams of ammonia are produced when you react 2.00 g of nitrogen with excess hydrogen. • N2 + 3 H2  2 NH3 2.00 g N2 1 mol N2 2 mol NH3 17.04 g NH3 28.02 g N2 1 mol N2 1 mol NH3 = 2.43 g NH3

  26. Practice Mass-Mole-Mass • How many grams of calcium nitride are produced when 2.00 g of calcium reacts with an excess of nitrogen? • Ca + N2 Ca3N2 • 3 Ca + N2 Ca3N2

  27. x 1 mol Ca3N2 x 148.26 g Ca3N2 3 mol Ca 1 mol Ca3N2 x 1 mol Ca 40.08 g Ca Mass-Mole-Mass • 3 Ca + N2 Ca3N2 2.00 g Ca = 2.47 g Ca3N2

  28. Some Things Just Take a Lot of Work!!!

  29. Stoichiometry : Mole Ratios to Determining Grams of ProductLet’s see if you can: • Review the conversion of particles or grams to moles • Determine mole ratios from a balanced chemical equation • Determine the amount of product produced when given the amount of reactants

  30. x 3 mol N2 x 28.02 g N2 2 mol NaN3 1 mol N2 x 1 mol NaN3 65.02 g NaN3 Mass-Mole-Mass • NaN3 Na + N2 • Decomposition • 2 NaN3 2 Na + 3 N2 • 65.02 g 22.99 g 28.02 g 94.5 g NaN3 = 61.1 g N2

  31. Don’t you just love these types of problems???

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