1. Honors Chemistry Final Exam Review

2. Good Luck!!!

3. Convert 15.2 m/s to km/hr 1. 54.7 km/hr 2. 0.912 km/hr 3. 4.22 km/hr 4. 5.47 x 10 7 5. not listed

4. Converting Word Equations into Chemical Equations Strontium iodide + Lead (II) phosphate  Strontium phosphate + lead (II) iodide SrI 2 + Pb 3 (PO 4 ) 2 ----> Sr 3 (PO 4 ) 2 + PbI 2 3 3

5. Practice Quiz Net Ionic Equations Write the molecular, complete ionic, and net ionic equations for this reaction: Silver nitrate reacts with calcium chloride Molecular: 2AgNO 3 + CaCl 2  2AgCl + Ca(NO 3 ) 2 Complete Ionic: 2Ag + + 2NO 3 - + Ca 2+ + 2Cl -  2AgCl + Ca 2+ + 2NO 3 - Net Ionic: 2Ag + + 2Cl -  2AgCl

6. Mixed Practice State the type, predict the products, and balance the following reactions: 1. BaCl 2 + H 2 SO 4  2. C 6 H 12 + O 2  3. Zn + CuSO 4  4. Cs + Br 2  5. FeCO 3  Double Displacement Combustion Single Displacement Synthesis Decomposition

7. Try This… Predict the products, balance the following reactions and show the change in oxidation numbers : Zinc reacts with aqueous copper (II) sulfate Zinc is higher relative activity so… Zn + CuSO 4  Cu + ZnSO 4 Each Zn loses 2e - oxidation, reducing agent Each Cu(II) gains 2e - reduction, oxidizing agent

8. Review Mass-Mole-Molecules: Determine the number of molecules in 73 g of water 73 g H 2 O # H 2 O molecules = x 1 mol H 2 O 18.02 g H 2 O = 2.4 x 10 24 molecules H 2 O x 6.02x10 23 molecules 1 mol H 2 O

9. Try this one: Calculate the mass in grams of iodine required to react completely with 0.50 moles of aluminum. Al + I 2  AlI 3 2 Al + 3 I 2  2 AlI 3 = 190 g I 2 0.50 mol Al x 3 mol I 2 2 mol Al x 253.80 g I 2 1 mol I 2

10. 0.50 g Al Try this one: Calculate the mass in grams of iodine required to react completely with 0.50 g of aluminum. Al + I 2  AlI 3 2 Al + 3 I 2  2 AlI 3 = 7.1 g I 2 x 3 mol I 2 2 mol Al x 253.80 g I 2 1 mol I 2 x 1 mol Al 26.98 g Al

11. x 3 mol Zn 2 mol MoO 3 What mass of ZnO is formed when 20.0 g of MoO 3 is reacted with 10.0 g of Zn? 20.0 g MoO 3 x 1 mol MoO 3 143.94 g MoO 3 3 Zn + 2 MoO 3  Mo 2 O 3 + 3 ZnO x 65.39 g Zn 1 mol Zn = 13.6 g Zn

12. x 3 mol ZnO 3 mol Zn What mass of ZnO is formed when 20.0 g of MoO 3 is reacted with 10.0 g of Zn? We need 13.6 g of Zn so Zn is limiting! 10.0 g Znx 1 mol Zn 65.39 g Zn 3 Zn + 2 MoO 3  Mo 2 O 3 + 3 ZnO x 81.39 g ZnO 1 mol ZnO = 12.4 g ZnO

13. x 118.00 g SbI 3 130.1 g SbI 3 Determine the percent yield if 118.00 g of antimony (III) iodide is produced. 130.1 g of Sbl 3 should have been produced. What is the percent yield? 2 Sb + 3 I 2  2 SbI 3 = 90.70 % Yield x 100

14. Empirical Formulas: 72% iron and 28% oxygen Determine the formula for this substance. moles of Fe 72 g Fe 55.85 g/mole = 1.29 moles Fe moles of O = 28 g O 16.00 g/mole = 1.75 moles O Formula:

15. Empirical Formulas #9: 72% iron and 28% oxygen Determine the formula for this substance. Multiply subscripts by 3 to get

16. How much water do I need to add to 250 mL of 3.0 M HCl to dilute it to 1.0 M HCl? = 0.75 L Total, therefore 0.50 L 3.0 M HCl x 0.250 L = 1.0 M HCl x L

17. Name HCl. 1. Hydrogen chloride 2. Hydrochloric acid 3. Chloric acid 4. Perchloric acid 5. Chlorous acid 6. Hypochlorus acid 7. I have no idea!! 8. Who cares??

18. Name HClO 4. 1. Hydrogen chloride 2. Hydrochloric acid 3. Chloric acid 4. Perchloric acid 5. Chlorous acid 6. Hypochlorus acid 7. I have no idea!! 8. Who cares??

19. Name Fe(OH) 3 1. Iron (III) Hydroxide 2. Iron Hydroxide 3. Ironic Acid 4. Iron (I) Hydroxide 5. Iron Oxyhydride 6. Not listed

20. Which of the following definitions of an acid includes conjugate acids? 1. Arrhenius 2. Bronsted-Lowry 3. Lewis 4. Kenzig 5. Woods 6. Toburen 7. Sabol 8. Sanson

21. Identify the conjugate base in the following equation. 1. NH 3 2. H 2 O 3. NH 4 + 4. OH-

22. H 2 O + CO 3 2-  OH - + HCO 3 According to Bronsted-Lowry theory, in the above reaction, H 2 O is a(n) 1. Acid 2. Base 3. Conjugate acid 4. Conjugate base

23. According to Lewis theory, PCl 3 is a(n) 1. Acid 2. Base 3. Salt 4. Conjugate Acid 5. Conjugate Base

24. The pOH of a 0.0030M solution of H 2 SO 4 is: 1. 2.52 2. 11.48 3. 2.22 4. 11.78 5. 0.99 6. 13.01

25. 100.0 mL of 3.000 M nitric acid neutralizes 3.000 M of aluminum hydroxide. How many mL of the base did you use? 1. 100.0 mL 2. 50.00 mL 3. 33.33 mL 4. 16.67 mL 5. 8.333 mL 6. Not listed

26. Learning Check A gas has a volume of 675 mL at 35°C and 0.850 atm pressure. What is the temperature in °C when the gas has a volume of 0.315 L and a pressure of 802 mm Hg?

27. Calculation P 1 = 0.850 atm V 1 = 675 mL T 1 = 308 K P 2 = 1.06 atm V 2 = 315 mL T 2 = ?? P 1 V 1 P 2 V 2 = P 1 V 1 T 2 = P 2 V 2 T 1 T 1 T 2 T 2 = 1.06 atm x 315 mL x 308 K 0.850 atm x 675 mL T 2 = 179 K - 273 = -94 °C = 179 K

28. Zinc will react with hydrochloric acid. The hydrogen gas is collected through water at 30.0 o C and 782 mm Hg. The vapor pressure of water at 30.0 o C is 32.0 mm Hg. What is the partial pressure of H 2 ? 1. 250 atm 2. 314 atm 3. 0.329 atm 4. 0.987 atm 5. Not listed

29. Zinc ( 65.39 g/mole) will react with hydrochloric acid. Determine the grams of zinc that must be reacted to produce this quantity of hydrogen if the volume is 142 mL. (P = 0.987 atm, T = 30.0 o C) 1. 0.112 g 2. 1.18 g 3. 628 g 4. 0.000 628 g 5. 0.369 g

30. When a gas forms a liquid, which process is taking place? 1. freezing 2. condensation 3. boiling 4. evaporation Chemical or Physical

31. Based on the melting points shown in the table, which material would still be a solid at 400°C? 1. beeswax 2. gold 3. lead 4. oxygen Based on the melting points shown in the table, which material would still be a solid at 400°C? 1. beeswax 2. gold 3. lead 4. oxygen Substance Melting Point (°C) Beeswax 62 Gold 1,063 Lead 327 Oxygen –218 Substance Melting Point (°C) Beeswax 62 Gold 1,063 Lead 327 Oxygen –218 Chemical or Physical

32. A chemical change for a piece of metal would be 1. being bent in half. 2. getting cut into two pieces. 3. being painted. 4. getting rusty.

33. States of Matter List the Location of Each Change of State Solid Liquid Gas Energy Melting DepositionFreezingSublimation CondensationBoiling Energy

34. List the Location of Each Enthapy Used to Change State Solid Liquid Gas Energy Heat of Fusion Heat of Vaporization Energy

35. Determine the energy released in joules as a 152.00 g sample of metal (0.0335 cal/g o C cools 51.5 o C q = c p x m x t: q = x J c p = 0.0335 cal/g o C (4.184 J/cal) m = 152.00 g t = -51.5 o C x = (0.140164 J/g o C )(152.00 g)(-51.5 o C) = -1.10 x 10 3 J

36. Zinc will react with hydrochloric acid. What are the 2 products for this reaction? 1. ZnCl + H 2. ZnCl + H 2 3. Zn 2 Cl + H 2 4. ZnCl 2 + H 2 5. Not listed

37. Zinc will react with hydrochloric acid. What kind of reaction is this? 1. DD 2. SD 3. Synthesis 4. Decomposition 5. Not listed

38. Zinc will react with hydrochloric acid. This reaction will form ZnCl 2 + H 2. What are the 4 coefficients for the balanced chemical equation? 1. 1,2,1,2 2. 2,1,2,1 3. 1,1,1,1 4. 2,2,1,2 5. Not listed

39. As you leave Chemistry always remember: You may not be perfect... but parts of you are excellent!!!

40. The End!!!