1. Stoichiometry Pronounced: Stoy-kee-AHM-uh-tree

2. What is stoichiometry? Its math that helps us to see the relationship between what is used and formed in a chemical reaction.

3. How do I do stoichiometry? Its just dimensional analysis.

4. What is the main key ingredient to stoichiometry? Mole ratios –Mole ratios are the way of getting from one part of the reaction to another

5. How do I get a mole ratio? Use the balanced equation. Oxygen reacts with hydrogen to make water.

6. Demo Copper reacts with Silver (I) Nitrate … Assume you have Cu +2 1.Predict your products. 2.Balance the rxn 3.Determine all the mole ratios that are possible

7. What will I be converting between in stoichiometry problems? Moles to moles Moles to grams Grams to moles Grams to grams

8. Mass of Given Moles of Given Molar Mass Mole Ratio Moles of Unknown Molar Mass Mass of Unknown

9. MOLES TO MOLES

10. NH 4 NO 3  N 2 O + H 2 O How many moles of H 2 O are produced if 3.65 moles of NH 4 NO 3 are decomposed?

11. Back to the Demo… If I began with 0.2583 moles of Cu, how many moles of Ag will form?

12. Again the Demo… If you have the same amount of Cu, how many moles of Copper (II) Nitrate will be made?

13. Determine how many moles of sodium chloride produced when 4.25 mol of chlorine gas reacts with sodium.

14. MOLES AND MASS

15. NaOH + H 2 SO 4  H 2 O + Na 2 SO 4 How many moles of sodium sulfate will be formed if you start with 222 grams of sodium hydroxide?

16. How many grams of H 2 and N 2 can be formed by the decomposition of 0.145 mol of ammonia, NH 3 ?

17. MASS TO MASS

18. Pb(SO 4 ) 2 + LiNO 3  Pb(NO 3 ) 4 + Li 2 SO 4 How many grams of lithium nitrate will be needed to make 5.2 grams of lithium sulfate?

19. Bromine reacts with sodium chloride to form chlorine and sodium bromide. If you begin with 73.2 g of sodium chloride, how many grams of chlorine will be produced

20. If you begin with 4.125g of iron(III)nitrate and react it with sodium hydroxide, how many grams of iron (III) hydroxide will you make in the end?

21. C 6 H 10 + O 2  CO 2 + H 2 O If I do this reaction with 45 grams of oxygen, how many grams of carbon dioxide will be formed?

22. Problem! You have 27 cars with out tires, and 55 tires. How many complete cars can you make?

23. What is a limiting reactant? It is finding out which reactant will be used up first in a problem

24. What does in excess mean? It means you have so much you will not run out when the reaction is completed..

25. What do you have to do for limiting reactant problems? Do 2 stoich problems

26. How do I set them up? Start with each of the reactants and take them to grams.

27. A 2.00 g sample of ammonia is mixed with 4.00 g of oxygen. Which is the limiting reactant? Which is in excess? NH 3(g) + O 2 (g)  NO (g) + H 2 O (g)

28. Which is the limiting reactant? The one that makes the LEAST amount of product.

29. How do you answer the 2 types of questions? If it asks what is the LR, your answer is one of your reactants. If it asks how much is made, your answer is the lower of the 2 amounts produced.

30. Is this why a reaction stops? Yes, one of the reactants is used up.

31. What mass of water can be produced by 4g of H 2 reacting with 16g of O 2 ?

32. 1)Write the balanced equation for the reaction of lead (II) nitrate with sodium iodide to form sodium nitrate and lead (II) iodide. 2)If I start with 25.0 grams of lead (II) nitrate and 15.0 grams of sodium iodide, how many grams of sodium nitrate can be formed? 3)What is the limiting reactant in the reaction described in problem 2?

33. What is percent yield? It is comparing how much yield you ACTUALLY get versus what you SHOULD get in the lab.

34. Is this different than Percent Error? YES! Percent error tells error in the lab, not the percent recovered.

35. What is the equation? Actualx100 Theoretical Actual is what you ACTUALLY got in the lab Theoretical is what you SHOULD have gotten in the lab

36. How do I find the theoretical? With a stoichiometry problem.

37. Zinc reacts with iodine to form zinc (II) iodide Calculate the theoretical yield if you start with 125.2g of zinc and 150.0g of iodine. Determine the percent yield if 215.6g of product is recovered.

38. CaCO 3  CaO + CO 2 Quicklime, CaO, can be prepared by roasting limestone, CaCO 3, according to the chemical equation below. When 2.00 x 10 3 g of CaCO 3 are heated, the actual yield of CaO is 1.50 x 10 3 g. What is the percent yield?