1. Stoichiometry The quantitative study of chemical reactions

2. Stoichiometric Steps Set up & balance rxn Change stuff given to moles Change moles given to ask Change what’s asked for to the proper unit

3. Step 1 Determine products of a reaction if they are not given Balance the reaction

4. Step 2 Use molar conversion to change whatever is given to moles

5. Step 3 Use the molar ratio from the balanced reaction to convert the moles of what is given to the moles of what’s asked for.

6. Step 4 Use molar conversions to change the moles of what is asked for to the proper unit

7. Calculate the volume of NH 3 formed at STP when 6.00 kg of H 2 react with excess N 2 to form NH 3

9. Calculate the mass of PbI 2 formed when 66.2 g of Pb(NO 3 ) 2 is combined with excess KI.

10. Calculate the number of molecules of oxygen gas required to burn 3.5 ng of C 5 H 10

11. Calculate the mass of MgCO 3 formed when 18.4 g of MgBr 2 is combined with a solution containing excess K 2 CO 3.

12. Calculate the volume of CO 2 formed at STP when 16.8 g of MgCO 3 is decomposed creating CO 2 & MgO.

13. Limiting Reactant The reactant that gets used up The reactant that determines the amount of product formed

14. Excess Reactant The reactant that does not get used up

15. Stoichiometry with Multiple Reagents Perform same steps for all reactants Choose least amount of product

16. Calculate the mass of glucose (C 6 H 12 O 6 ) formed when 880 g of carbon dioxide is combined with 720 g of water in photosynthesis

17. Calculate the # of molecules of NH 3 formed when 4.0  g of H 2 react with 1.12 mL of N 2 gas at STP.

18. Theoretical Yield The amount determined through stoichiometry The amount solved for on paper

19. Experimental Yield The amount obtained in the lab Actual yield

20. Percent yield % Yield = (Exp/Theo) x 100 %

21. 68 g NH 3 was obtained in lab when 140 g of N 2 reacts with excess H 2. Calculate percent yield.

22. 510 g PH 3 were obtained in the lab when 0.62 kg of P 4 reacted with excess H 2. Calculate percent yield.

23. Determine the volume of O 2 released at STP when 32 kg of Fe 2 O 3 is purified with an 80.0 % yield making Fe & O 2

24. Calculate the volume of oxygen gas at STP required to burn 12 kg of erythrose (C 4 H 8 O 4 )

25. Calculate the mass of BaSO 4 formed when 41.6 g of BaCl 2 is added to 17.4 g K 2 SO 4 giving a 50.0 % yield:

26. Calculate the mass of CaSO 4 formed when 2.00 g of calcium bromide is added to 75 mL of 0.40 M sodium sulfate:

27. Terms: Stoichiometry Percent yield Limiting Reactant Excess reactant Theoretical yield Experimental yield

28. Calculate the volume in mL of oxygen gas at STP required to burn 50.0 mg C 5 H 8 O 2 :

29. 3.67 g of PbBr 2 was obtained in lab when 6.62 g of Pb(NO 3 ) 2 was added to 11.9 g KBr. Calculate the % yield.

30. Calculate the volume of gaseous product formed when 4.2 kg of MgCO 3 is heated with a 75 % yield: MgCO 3  MgO + CO 2

31. Calculate the volume of Cl 2 collected at STP when 3.80  g of F 2 at STP is bubbled through a 0.050 mL solution of 0.020 M KCl:

32. Calculate the volume in mL of gaseous products formed at STP when 6.0  g of C 2 H 6 is burned in excess oxygen:

33. 33.1 g of Pb(NO 3 ) 2 was added to 1500 mL 0.10 M KI. Calculate mass of PbI 2 formed.

34. Chm II: Calculate the mass of water & NaCl formed when 6.0 g of sodium hydroxide is added to a 250 mL solution 0.40 M hydrochloric acid:

35. Chm II: 33.1 g of Pb(NO 3 ) 2 was added to 1500 mL 0.10 M KI. Calculate mass of PbI 2 formed.

36. Chm II: 29.7 g of BaBr 2 was added to 1500 mL 0.10 M K 2 SO 4. Calculate mass of BaSO 4 formed.

37. An 30.0 g unknown sample (containing only C, H, & O) was burned in excess oxygen yielding 66 g CO 2 & 36 g H 2 O. Calculate its empirical formula :

38. An 240 g unknown sample (containing only C, H, S, & O) was burned in excess oxygen yielding 352 g CO 2, 144 g H 2 O, & 128 g, SO 2. Calculate its empirical formula :

39. Calculate the mass of solid product formed when 3.31 g of Pb(NO 3 ) 2 is added to a 75.0 mL solution 0.20 M KI:

40. Name the Following: BaCl 2 Mn 2 O 3 SF 2 NH 3 CaSO 4 (NH 4 ) 3 PO 3 Fe(NO 3 ) 2 KClO 3

41. Derive formulas for Sodium hydroxide Calcium carbonate Iron(III)phosphate Dinitrogen tetroxide

42. Make conversions: 64 kg SO 2 to mL gas 11.2  L NH 3 to atoms 180 km/hr to cm/s