1. 1 Session 4: Stoichiometry I Tom Hsu, PhD. Manos Chaniotakis, PhD. Marina Dang, PhD. Copyright © 2012 Chaniotakas and Hsu

2. How do we define and measure chemical quantities? –Do we count atoms? –Do we count moles? –Do we measure in grams? –Do we measure in liters? Essential questions

3. Write a balanced chemical equation for a reaction. Calculate the number of moles of products and reactants. Translate reaction quantities from moles to grams. Identify any limiting reactants. Apply the concepts to design a stoichiometric reaction to produce a specified quantity of product. Objectives

4. 8 (A) define and use the concept of a mole; 8 (D) use the law of conservation of mass to write and balance chemical equations; and 8 (E) perform stoichiometric calculations, including determination of mass relationships between reactants and products, calculation of limiting reagents, and percent yield. TEKS

5. Consider the above chemical reaction. 1.How many moles of sodium bicarbonate react to form one mole of carbon dioxide? 2.If 1 gram of CO 2 is produced, how many grams of sodium bicarbonate were reacted? 3.Calculate the the mass of vinegar needed to completely react with 5 grams of sodium bicarbonate. Assessment

6. Setting up the reaction 1.Put an empty cup on the balance and zero it. Measure 10.0 g of baking soda in the cup. Record the measured mass in Table 1. 2.Put another empty cup on the balance and zero it. Measure 30.0 g of vinegar in the cup. Record the measured mass in Table 1. 3.Add the masses of vinegar and baking soda. Record the sum in Table 1 (row 3).

7. Doing the reaction Slowly pour the vinegar into the baking soda. Pouring it too fast might cause the bubbling to overflow! Wait until the bubbling has stopped and record the mass.

8. Observations a.What evidence did you observe that indicated a chemical reaction was taking place? b.Explain the difference in the total mass before and after mixing. c.Do you see any baking soda that has not reacted?

9. Work out the formula masses The balanced reaction is written on the first line of the chart above. Calculate the formula mass of each of the products and reactants. Baking soda (sodium bicarbonate) Acetic acid (acid in vinegar)

10. Work out the formula masses One of the products is a gas. Which one? Will this product’s mass contribute to the mass as measured on the balance after the reaction has finished? Why or why not? On the second line, write down the mass of the baking soda and vinegar you added. Baking soda (sodium bicarbonate) Acetic acid (acid in vinegar) 84.00 60.0582.03 44.0018.01

11. Calculate moles of reactants Use the formula masses to calculate the number of moles of NaHCO 3 and HC 2 H 3 O 2. 84.00 60.0582.03 18.0144.00 Vinegar is 5% acetic acid (HC 2 H 3 O 2 ) by mass. Multiply by 0.05 to get the actual mass of acetic acid.

12. Calculate moles of products How many moles of CO 2 were produced? Use the formula mass to calculate the mass of CO 2 produced. 84.00 60.0582.03 18.0144.00

13. Calculate moles of products Compare the mass of CO 2 you calculated with the mass difference you measured from your experiment. Does this explain the “missing” mass? According to your calculations, did all the baking soda react? Is this consistent with your observations? What was the limiting reactant in this experiment?

14. Calculate moles of products To make an efficient reaction, there should not be any reactants left over. Use this chart to calculate how many grams of vinegar need to be added to react completely with 10 grams of baking soda. 84.00 60.05

15. Test your predictions Measure out 10.0 g of baking soda in one cup. Measure out the required amount of vinegar (from your calculations) in the other cup. Write down the total mass before you mix the reactants.

16. Do the reaction Slowly pour the vinegar into the baking soda. Pouring it too fast might cause the bubbling to overflow! Wait until the bubbling has stopped and record the mass.

17. Test your predictions Calculate the mass of CO 2 produced. How does this number match your experiment? 84.0060.0582.0344.0018.01

18. Chemical manufacturing Commodity manufacturers usually take inexpensive raw materials and make a chemical product in a single-purpose factory. Gasoline Polyethylene and other plastics Cement Ammonium nitrate fertilizer Specialty manufacturers have a general-purpose factory that may produce batches of many different compounds. Medical compounds Dyes Paints Foods and food additives

19. Portland Cement A hydraulic material which hardens and becomes insoluble when hydrated. The main ingredient in concrete, mortar, and stucco. Manufactured from limestone and clay or shale. Cement (major components) 50% Ca 3 SiO 5 25% Ca 2 SiO 4 10% Ca 3 Al 2 O 6 10% Ca 4 Al 12 Fe 2 O 10 Cement (major components) 50% Ca 3 SiO 5 25% Ca 2 SiO 4 10% Ca 3 Al 2 O 6 10% Ca 4 Al 12 Fe 2 O 10 Jubilee Church, Rome

20. Manufacturing chemistry Limestone ( CaCO 3 ) Shale ( SiO 2 + Al 2 O 3 + Fe 2 O 3 ) Limestone ( CaCO 3 ) Shale ( SiO 2 + Al 2 O 3 + Fe 2 O 3 ) Cement 50% Ca 3 SiO 5 25% Ca 2 SiO 4 10% Ca 3 Al 2 O 6 10% Ca 4 Al 12 Fe 2 O 10 Cement 50% Ca 3 SiO 5 25% Ca 2 SiO 4 10% Ca 3 Al 2 O 6 10% Ca 4 Al 12 Fe 2 O 10 Reactants Products

21. Making CO 2 What ingredients do you need to manufacture 10 grams of carbon dioxide using the reaction of sodium bicarbonate and acetic acid?

22. Making CO 2 What ingredients do you need to manufacture 10 grams of carbon dioxide using the reaction of sodium bicarbonate and acetic acid? This is a dumb way to do this, but instructionally useful!

23. Making CO 2 84.00 60.0582.03 44.0018.01

24. Making CO 2 84.00 60.0582.03 44.0018.01 0.23

25. Making CO 2 84.0060.05 82.0344.00 18.01 0.23

26. Making CO 2 84.00 60.0582.03 44.0018.01 0.23 19.3 g

27. Making CO 2 84.00 60.0582.03 44.0018.01 0.23 19.3 g 13.8 g 276 g

28. Perfect combustion of octane: If the fuel is burned perfectly, the reaction that occurs in a gasoline engine would only produce carbon dioxide and water.

29. Perfect combustion of octane: a.Calculate the formula mass for octane. b.Suppose a car uses 25 gallons of gasoline in a week. The density of gasoline is about 2,900 g/gallon. Calculate the mass in grams of 25 gallons of gasoline.

30. Perfect combustion of octane: a.Calculate the formula mass for octane. 114.2 g b.Suppose a car uses 25 gallons of gasoline in a week. The density of gasoline is about 2,900 g/gallon. Calculate the mass in grams of 25 gallons of gasoline. 72,500 g

31. Perfect combustion of octane: c. Assume gasoline is pure octane. How many moles does this quantity represent? d. How many moles of CO 2 are created for every 2 moles of gasoline burned? e. Calculate the mass of CO 2 released from the perfect combustion of 25 gallons of gasoline.

32. Perfect combustion of octane: c. Assume gasoline is pure octane. How many moles does this quantity represent? 635 d. How many moles of CO 2 are created for every mole of gasoline burned? 8 e. Calculate the mass of CO 2 released from the perfect combustion of 25 gallons of gasoline. 5,080 mol = 223,520 g (223.5 kg)

33. Perfect combustion of octane: c. Assume gasoline is pure octane. How many moles does this quantity represent? 635 d. How many moles of CO 2 are created for every mole of gasoline burned? 8 e. Calculate the mass of CO 2 released from the perfect combustion of 25 gallons of gasoline. 5,080 mol = 223,520 g (223.5 kg) from 72.5 kg of gas

34. Perfect combustion of octane: c. Assume gasoline is pure octane. How many moles does this quantity represent? 635 d. How many moles of CO 2 are created for every mole of gasoline burned? 8 e. Calculate the mass of CO 2 released from the perfect combustion of 25 gallons of gasoline. 5,080 mol = 114,000 liters = 114 m3 = 30 car volumes

35. Big ideas On the atomic level, elements combine by moles, not grams. For example, 2 hydrogen atoms per oxygen atom in H 2 O. We cannot measure moles but we can measure grams. Stoichiometry is the process of converting the quantities in moles from a balanced reaction into measurable quantities in grams.

36. Assessment Consider the above chemical reaction. 1.How many moles of sodium bicarbonate react to form one mole of carbon dioxide?

37. Assessment Consider the above chemical reaction. 1.How many moles of sodium bicarbonate react to form one mole of carbon dioxide? One

38. Assessment Consider the above chemical reaction. 2.If 1 gram of CO 2 is produced, how many grams of sodium bicarbonate were reacted?

39. Assessment Consider the above chemical reaction. 2.If 1 gram of CO 2 is produced, how many grams of sodium bicarbonate were reacted?

40. Assessment Consider the above chemical reaction. Calculate the the mass of vinegar needed to completely react with 5 grams of sodium bicarbonate.

41. Assessment Consider the above chemical reaction. Calculate the the mass of vinegar needed to completely react with 5 grams of sodium bicarbonate.

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