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Bell Ringer

Bell Ringer. Aluminum + Sulfuric Acid  Aluminum Sulfate + Hydrogen Gas. Which of the following is the balanced chemical equation for the reaction shown above?. A Al + H 2 SO 4  Al 2 (SO 4 ) 3 + H 2.

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Bell Ringer

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  1. Bell Ringer Aluminum + Sulfuric Acid  Aluminum Sulfate + Hydrogen Gas Which of the following is the balanced chemical equation for the reaction shown above? A Al + H2SO4Al2(SO4)3 +H2 B 2Al +3H2SO4Al2(SO4)3 +3H2 C 2Al +3H2SO4Al2(SO4)3 +H2 D 2Al +H2SO4Al2(SO4)3 +H2 2004 SOL

  2. Nerf & Poof Factor Method CONVERSION FACTORS: 1 nerf = 3 poof 5 splunk = 6 mews 2 poof = 7 splat 2 pock = 3 splunk 4 trad = 1 pock 8 splat = 3 trad • 6 nerf = ? trad • 3.6 mews = ? pock • 7 poof = ? nerf • 3 mol Na2P = ?atoms Na

  3. 2.25 cups flour 8 Tbsp butter 0.5 cups shortening 0.75 cups sugar 0.75 cups brown sugar 1 tsp salt 1 tsp baking soda 1 tsp vanilla 0.5 cups Egg Beaters Chocolate Chip Cookies

  4. 2.25cupsflour 8Tbspbutter 0.5cupsshortening 0.75cupssugar 0.75cupsbrown sugar 1tspsalt 1tspbaking soda 1tspvanilla 0.5cupsEgg Beaters How much? Of what? What units? Chocolate Chip Cookies

  5. How much? Of what? Chocolate Chip Cookies • 2.25flour • 8butter • 0.5shortening • 0.75sugar • 0.75brown sugar • 1salt • 1baking soda • 1vanilla • 0.5Egg Beaters

  6. How much? What units? Chocolate Chip Cookies • 2.25cups • 8Tbsp • 0.5cups • 0.75cups • 0.75cups • 1tsp • 1tsp • 1tsp • 0.5cups

  7. How much? Of what? What units? Chocolate Chip Cookies • 2.25cupsflour • 8Tbspbutter • 0.5cupsshortening • 0.75cupssugar • 0.75cupsbrown sugar • 1tspsalt • 1tspbaking soda • 1tspvanilla • 0.5cupsEgg Beaters

  8. Get on with it! What does this have to do with CHEMISTRY?

  9. (177ºC) 1 batch of chocolate chip cookies! 2.25 cups flour + 8 Tbsp butter + 0.5 cups shortening + 0.75 cups sugar + 0.75 cups brown sugar + 1 tsp salt + 1 tsp baking soda + 1 tsp vanilla + 0.5 cups Egg Beaters unit substance coefficient (a synthesis reaction)

  10. Welcome to STOICHIOMETRY Mr. Trotts 2008

  11. What is Stoichiometry? • The study of quantitative relationships within chemical reactions • A balanced equation is the key to stoichiometry! • Tools you’ll need for this chapter: • Writing proper formulas and balanced reactions • Converting from mass to moles and vice versa

  12. Let’s Revisit the Cookies… For 1 batch: The Egg Beaters I have are close to expiring! I’d like to use the rest of them in this recipe. I have 1.5 cups of Egg Beaters. • 2.25 cups flour • 8 Tbsp butter • 0.5 cups shortening • 0.75 cups sugar • 0.75 cups brown sugar • 1 tsp salt • 1 tsp baking soda • 1 tsp vanilla • 0.5 cups Egg Beaters How many batches of cookies can I make with that many Egg Beaters?

  13. Let’s Revisit the Cookies… For 1 batch: I have 1.5 cups of Egg Beaters. • 2.25 cups flour • 8 Tbsp butter • 0.5 cups shortening • 0.75 cups sugar • 0.75 cups brown sugar • 1 tsp salt • 1 tsp baking soda • 1 tsp vanilla • 0.5 cups Egg Beaters How many batches of cookies can I make with that many Egg Beaters? 1 batch cookies 1.5 cups E.B. x = 0.5 cups E.B. 3.0 batches of cookies

  14. Let’s Revisit the Cookies… For 1 batch: I have 1.5 cups of Egg Beaters. • 2.25 cups flour • 8 Tbsp butter • 0.5 cups shortening • 0.75 cups sugar • 0.75 cups brown sugar • 1 tsp salt • 1 tsp baking soda • 1 tsp vanilla • 0.5 cups Egg Beaters How much butter do I need to deplete (use up) the Egg Beaters? 8 Tbsp butter 1.5 cups E.B. x = 0.5 cups E.B. 24 Tablespoons of butter

  15. … Back to Chemistry • There are three types of stoichiometry problems we will deal with today: • Mole-Mole problems (1 conversion) • Mass-Mole problems (2 conversions) • Mass-Mass problems (3 conversions) given required

  16. Baby Steps… Mole-Mole Problems • Step 1: Write a BALANCED EQUATION • Step 2: Determine the mole ratio from the coefficients in the equation. • Mole ratio = moles of required substance moles of given substance • Step 3: Set up the problem like a unit conversion and solve!

  17. Mole-Mole Problems Example: 2 H2O 2 H2 + O2 How many moles of water can be formed from 0.5 mol H2? 2 mol H2O 0.5 mol H2 0.5 mol H2O x = 2 mol H2

  18. 3 2 3 Mole-Mole Practice ? mol 0.5 mol ? mol ? mol CuSO4 + Al Al2(SO4)3 + Cu Mole ratio 3 mol CuSO4 1. a. 0.5 mol Al 0.8 mol CuSO4 x = 2 mol Al 1 mol Al2(SO4)3 b. 0.5 mol Al 0.3 mol Al2(SO4)3 x = 2 mol Al 3 mol Cu c. 0.5 mol Al 0.8 mol Cu x = 2 mol Al

  19. #2) Ca + AlCl3 CaCl2 + Al • Balance the formula • Given 2.5 moles Ca find the number of moles of AlCl3, CaCl2, and Al needed.

  20. 3 2 2 Mole-Mole Practice Ca + AlCl3 3 CaCl2 + Al 2 mol AlCl3 2. a. 2.5 mol Ca 1.7 mol AlCl3 x = 3 mol Ca 3 mol CaCl2 b. 2.5 mol Ca 2.5 mol CaCl2 x = 3 mol Ca 2 mol Al c. 2.5 mol Ca 1.7 mol Al x = 3 mol Ca

  21. complete the mole to mole worksheet Do not write on the handout!!

  22. Quiz: mole to mole • 5 moles of Ca(OH)2 is added to a container of HCl in an attempt to neutralize the acid. How many moles of the HCl will be neutralized as CaCl2 and water are produced? Show your work for credit to include the molar ratio.

  23. Mass-Mole Problems • Step 1: Write a BALANCED EQUATION • Step 2: Calculate the molar mass of your given substance and convert from mass to moles • Step 3: Determine the mole ratio from the coefficients in the equation • Step 4: Set up the conversion and solve!

  24. Mass-Mole Problems Example: 2 H2O 2 H2 + O2 How many moles of water can be formed from 48.0 g O2? 1 mol O2 2 mol H2O 48.0 g O2 3.00 mol H2O x x = 32.00 g O2 1 mol O2

  25. 3 2 3 Mass-Mole Practice ? mol 13.5 g ? mol ? mol CuSO4 + Al Al2(SO4)3 + Cu Mole ratio 1 mol Al 3 mol CuSO4 3a. 13.5 g Al 0.751 mol CuSO4 x x = 26.98 g Al 2 mol Al 1 mol Al 1 mol Al2(SO4)3 b. 13.5 g Al x x 0.250 mol Al2(SO4)3 = 26.98 g Al 2 mol Al 1 mol Al 3 mol Cu c. 13.5 g Al x 0.751 mol Cu x = 26.98 g Al 2 mol Al

  26. #4 Ca + AlCl3 CaCl2 + Al • Balance the equation • Given 5.7 g of Calcium find the number of moles of AlCl3, CaCl2, and Al

  27. 3 2 2 Mass-Mole Practice Ca + AlCl3 3 CaCl2 + Al 1 mol Ca 2 mol AlCl3 4. a. 5.7 g Ca x x 0.095 mol AlCl3 = 40.08 g Ca 3 mol Ca 1 mol Ca 3 mol CaCl2 b. 5.7 g Ca x x 0.14 mol CaCl2 = 40.08 g Ca 3 mol Ca 1 mol Ca 2 mol Al c. 5.7 g Ca x x 0.095 mol Al = 40.08 g Ca 3 mol Ca

  28. Mass-Mass Problems Example: 2 H2O 2 H2 + O2 How many grams of water can be formed from 48.0 g O2? 1 mol O2 2 mol H2O 18.02 g H2O 48.0 g O2 54.1 g H2O x x x = 32.00 g O2 1 mol O2 1 mol H2O

  29. 3 2 3 Mass-Mass Practice ? g ? g ? g 8.5 g CuSO4 + Al Al2(SO4)3 + Cu Mole ratio 1 mol Al 3 mol CuSO4 159.61 g CuSO4 5. a. 8.5 g Al = x x x 26.98 g Al 2 mol Al 1 mol CuSO4 75 g CuSO4 1 mol Al 1 mol Al2(SO4)3 342.14 g Al2(SO4)3 b. 8.5 g Al x x x = 26.98 g Al 2 mol Al 1 mol Al2(SO4)3 54 g Al2(SO4)3

  30. Mass-Mass Practice 1 mol Al 3 mol Cu 63.55 g Cu c. 8.5 g Al x x x = 26.98 g Al 2 mol Al 1 mol Cu 30. g Cu

  31. #6a. How many grams of aluminum chloride would be required to completely react with 1.9 grams of Calcium? #6b. How many grams of Calcium chloride will be produced from 1.9 grams of Calcium? #6c. How many grams of Aluminum will be produced from 1.9 grams of Calcium?

  32. 3 2 2 Mass-Mass Practice Ca + AlCl3 3 CaCl2 + Al 1 mol Ca 2 mol AlCl3 133.33 g AlCl3 6. a. 1.9 g Ca x x x = 40.08 g Ca 3 mol Ca 1 mol AlCl3 4.2 g AlCl3 1 mol Ca 3 mol CaCl2 110.98 g CaCl2 b. 1.9 g Ca x x x = 40.08 g Ca 3 mol Ca 1 mol CaCl2 5.3 g CaCl2

  33. 3 2 2 Mass-Mass Practice Ca + AlCl3 3 CaCl2 + Al 1 mol Ca 2 mol Al 26.98 g Al c. 1.9 g Ca x x x = 40.08 g Ca 3 mol Ca 1 mol Al 0.85 g Al

  34. Now complete the Mass to Mass handout Do not write on the handout

  35. Quiz 7. 7.5 moles of potassium phosphate is reacted with excess barium chloride. How many grams of potassium chloride are produced in the reaction? Write a balanced equation Use the equation and molar ratios to solve the problem

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