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 + H 2 SO 4   Al 2 (SO 4 ) 3 + H 2 B 2Al + 3H 2 SO 4   Al 2 (SO 4 ) 3 + 3H 2 C 2Al + 3H 2 SO 4   Al 2 (SO 4 ) 3 + H 2 D2Al + H 2 SO 4   Al 2 (SO 4 ) 3 + H 2 2004 SOL

3. Nerf & Poof Factor Method CONVERSION FACTORS: 1 nerf = 3 poof5 splunk = 6 mews 2 poof = 7 splat2 pock = 3 splunk 4 trad = 1 pock8 splat = 3 trad 1.6 nerf = ? trad 2.3.6 mews = ? pock 3.7 poof = ? nerf 4.3 mol Na 2 P = ?atoms Na

4. 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

5. 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 How much? What units? Of what?

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

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

8. 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 How much? What units? Of what?

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

10. 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 (a synthesis reaction) (177ºC) 1 batch of chocolate chip cookies! coefficient unit substance

11. Welcome to STOICHIOMETRY Mr. Trotts 2008

12. 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

13. Let’s Revisit the 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 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. How many batches of cookies can I make with that many Egg Beaters?

14. Let’s Revisit the 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 For 1 batch: I have 1.5 cups of Egg Beaters. How many batches of cookies can I make with that many Egg Beaters? 1.5 cups E.B. x 1 batch cookies 0.5 cups E.B. = 3.0 batches of cookies

15. Let’s Revisit the 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 For 1 batch: I have 1.5 cups of Egg Beaters. How much butter do I need to deplete (use up) the Egg Beaters? 1.5 cups E.B. x 8 Tbsp butter 0.5 cups E.B. = 24 Tablespoons of butter

16. … 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

17. 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! Baby Steps… Mole-Mole Problems

18. Mole-Mole Problems Example: 2 H 2 + O 2 2 H 2 O How many moles of water can be formed from 0.5 mol H 2 ? 0.5 mol H 2 x 2 mol H 2 2 mol H 2 O = 0.5 mol H 2 O

19. Mole-Mole Practice CuSO 4 AlAl 2 (SO 4 ) 3 Cu323 ++ 1. a.0.5 mol Al 3 mol CuSO 4 2 mol Al =x 0.8 mol CuSO 4 b. c. 0.5 mol Al 1 mol Al 2 (SO 4 ) 3 2 mol Al =x 0.3 mol Al 2 (SO 4 ) 3 0.5 mol Al 3 mol Cu 2 mol Al =x 0.8 mol Cu Mole ratio 0.5 mol? mol

20. #2) Ca + AlCl 3 CaCl 2 + Al 1.Balance the formula 2.Given 2.5 moles Ca find the number of moles of AlCl 3, CaCl 2, and Al needed.

21. Mole-Mole Practice 2. a. 2.5 mol Ca 2 mol AlCl 3 3 mol Ca =x 1.7 mol AlCl 3 b. c. 2.5 mol Ca 3 mol CaCl 2 3 mol Ca =x 2.5 mol CaCl 2 2.5 mol Ca 2 mol Al 3 mol Ca =x 1.7 mol Al CaAlCl 3 CaCl 2 Al322 ++ 3

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

23. 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 CaCl 2 and water are produced? Show your work for credit to include the molar ratio.

24. 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!

25. Mass-Mole Problems Example: 2 H 2 + O 2 2 H 2 O How many moles of water can be formed from 48.0 g O 2 ? 48.0 g O 2 x 1 mol O 2 2 mol H 2 O = 3.00 mol H 2 O 32.00 g O 2 1 mol O 2 x

26. Mass-Mole Practice CuSO 4 AlAl 2 (SO 4 ) 3 Cu323 ++ 3a.13.5 g Al 1 mol Al 26.98 g Al =x 0.751 mol CuSO 4 b. c. 13.5 g Al 1 mol Al 2 (SO 4 ) 3 2 mol Al = x0.250 mol Al 2 (SO 4 ) 3 13.5 g Al 3 mol Cu 2 mol Al = x0.751 mol Cu Mole ratio x 3 mol CuSO 4 2 mol Al 1 mol Al 26.98 g Al x 1 mol Al 26.98 g Al x 13.5 g? mol

27. #4 Ca + AlCl 3 CaCl 2 + Al 1.Balance the equation 2.Given 5.7 g of Calcium find the number of moles of AlCl 3, CaCl 2, and Al

28. Mass-Mole Practice 4. a.5.7 g Ca 2 mol AlCl 3 3 mol Ca = x0.095 mol AlCl 3 b. c. 5.7 g Ca 3 mol CaCl 2 3 mol Ca = x0.14 mol CaCl 2 5.7 g Ca 2 mol Al 3 mol Ca = x0.095 mol Al CaAlCl 3 CaCl 2 Al322 ++ 1 mol Ca x x x 40.08 g Ca 1 mol Ca 40.08 g Ca 1 mol Ca 40.08 g Ca 3

29. Mass-Mass Problems Example: 2 H 2 + O 2 2 H 2 O How many grams of water can be formed from 48.0 g O 2 ? 48.0 g O 2 x 1 mol O 2 2 mol H 2 O = 32.00 g O 2 1 mol O 2 xx 18.02 g H 2 O 1 mol H 2 O 54.1 g H 2 O

30. Mass-Mass Practice CuSO 4 AlAl 2 (SO 4 ) 3 Cu323 ++ 5. a.8.5 g Al 1 mol Al 26.98 g Al = x 75 g CuSO 4 b.8.5 g Al 1 mol Al 2 (SO 4 ) 3 2 mol Al = x 54 g Al 2 (SO 4 ) 3 Mole ratio x 3 mol CuSO 4 2 mol Al 1 mol Al 26.98 g Al x 1 mol CuSO 4 342.14 g Al 2 (SO 4 ) 3 1 mol Al 2 (SO 4 ) 3 x x 159.61 g CuSO 4 8.5 g? g

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

32. #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?

33. Mass-Mass Practice 6. a.1.9 g Ca 2 mol AlCl 3 3 mol Ca = x 4.2 g AlCl 3 b.1.9 g Ca 3 mol CaCl 2 3 mol Ca = x 5.3 g CaCl 2 CaAlCl 3 CaCl 2 Al322 ++ 1 mol Ca x x 40.08 g Ca 1 mol Ca 40.08 g Ca x 133.33 g AlCl 3 1 mol AlCl 3 x 1 mol CaCl 2 110.98 g CaCl 2 3

34. Mass-Mass Practice c.1.9 g Ca 2 mol Al 3 mol Ca = x 0.85 g Al x 1 mol Ca 40.08 g Ca1 mol Al 26.98 g Al x CaAlCl 3 CaCl 2 Al322 ++ 3

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

36. 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