1. Jeopardy

2. Review Unit 3 Final Jeopardy 300 500 400 100 Counting Particles 200 300 400 500 100 200 400 300 500 200 300 400 500 100 200 300 400 500 100 200 Chemical Rxns Stoichiometry Mole Stuff Avogadro & His Number PLUS MORE! 600 100 600

3. Mole Stuff 100 What is a mole?

4. Mole Stuff 100 - Answer A volumetric unit of measure. One mole has as many particles in it as Avogadro’s number.

5. Mole Stuff 200 What is the molar mass? How do you find it?

6. Mole Stuff 200 - Answer The molar mass is the mass of one mole of substance. It can be found by reading the atomic masses on the periodic table.

7. Mole Stuff 300 What is relative mass? How is it connected to the Periodic Table?

8. Mole Stuff 300 - Answer Relative masses are masses relative to the smallest mass available. The atomic masses on the Periodic Table are all relative to Hydrogen.

9. Mole Stuff 400 What is the molar mass of potassium oxide?

10. Mole Stuff 400 - Answer K 2 O 39 g/mol + 39 g/mol + 16 g/mol 94 g/mol

11. Mole Stuff 500 How many moles are in a 12.0 g sample of iron (III) oxide?

12. Mole Stuff 500 - Answer 0.075 moles Fe 2 O 3 Molar mass Fe 2 O 3 : 159.6 g/mol (12g) * (1mol/159.6g) = 0.075 mol

13. Mole Stuff 600 What is the mass of 0.015 moles of calcium hydroxide?

14. Mole Stuff 600 - Answer 1.11 grams Ca(OH) 2 Molar Mass Ca(OH) 2 : 74 g/mol (0.015mol) * (74g/1mol) = 1.11 g

15. Avogadro & His Number 100 What is Avogadro’s Number? What does it mean?

16. Avogadro & His Number 100 - Answer 6.02 x 10 23 This is how many particles are in one mole of substance

17. Avogadro & His Number 200 How many silver atoms are contained in 0.650 grams of silver?

18. Avogadro & His Number 200 - Answer 3.63 x 10 21 atoms (0.65g) * (1mol/107.9g) * (6.02x10 23 part/1mol) = 3.63 * 10 21 particles

19. Avogadro & His Number 300 How many atoms are in 0.450 gram of iron?

20. Avogadro & His Number 300 - Answer 4.86 x 10 21 atoms Fe

21. Avogadro & His Number 400 How many molecules are in 13.2 grams of carbon dioxide?

22. Avogadro & His Number 400 - Answer 1.81 x 10 23 molecules CO 2

23. Avogadro & His Number 500 How many H 2 molecules are there in 0.25 moles of H 2 ?

24. Avogadro & His Number 500 - Answer 1.5 x 10 23 particles H 2

25. Avogadro & His Number 600 How many O atoms in 0.456 moles of AgNO 3 ?

26. Avogadro & His Number 600 - Answer 8.24 x 10 23 O atoms

27. Counting Particles 100 How many oxygen atoms are represented by the formula Pb(C 2 O 4 ) 2 ?

28. Counting Particles 100 - Answer 8

29. Counting Particles 200 What is total number of atoms represented by the formula Fe 2 (SO 4 ) 3 ?

30. Counting Particles 200 - Answer 17

31. Counting Particles 300 A 9.56 g sample of copper (II) sulfide is found to contain 6.35 g of copper. What is the percent by mass of the copper and sulfur in this compound?

32. Counting Particles 300 - Answer 66.4% Cuand33.6% S (6.35gCu/9.65g)*100% = 66.4% (3.21gS/9.65g)*100% = 33.6%

33. Counting Particles 400 Given the diagram of the molecule below, write the empirical and molecular formulas. Label each.

34. Counting Particles 400 - Answer Molecular: C 2 H 6 Empirical: CH 3

35. Counting Particles 500 When 0.062 g of phosphorus burns in air, it forms 0.142 g of phosphorus oxide. Determine the empirical formula of phosphorus oxide.

36. Counting Particles 500 - Answer P 2 O 5 Convert mass to molesRatio of Moles Whole # (0.062g P)*(1mol P/31g P) = 0.002mol P 1x2 = 2 (0.08g O)*(1mol O/16g O) = 0.005mol O 2.5x2 = 5

37. Counting Particles 600 What is the molecular formula of each compound? Empirical FormulaActual Molar Mass of Compound CH78 g/mole NO292 g/mole

38. Counting Particles 600 - Answer C6H6N2O4C6H6N2O4

39. Chemical Rxns 100 Balance the following reaction: __Sr(OH) 2 + __FeCl 3  __SrCl 2 + __Fe(OH) 3

40. Chemical Rxns 100 - Answer 3 Sr(OH) 2 + 2 FeCl 3  3 SrCl 2 + 2 Fe(OH) 3

41. Chemical Rxns 200 What type of reaction is the following? C 2 H 4 + 3O 2 –> 2CO 2 + 2H 2 O

42. Chemical Rxns 200 - Answers COMBUSTION REACTION boom!

43. Chemical Rxns 300 A reaction takes place in a test tube. You feel the bottom of the tube and it feels warm. Is the reaction exothermic or endothermic? WHY?

44. Chemical Rxns 300 - Answer EXOTHERMIC The system is releasing heat to the surroundings – energy is exiting the system and moving into your hand.

45. Chemical Rxns 400 Write a balanced chemical reaction for the reaction below: Magnesium hydroxide reacts with nitric acid (HNO 3 ) to form water and magnesium nitrate.

46. Chemical Rxns 400 - Answer Mg(OH) 2 + 2 HNO 3  2 H 2 O + Mg(NO 3 ) 2

47. Chemical Rxns 500 What is the formula of the missing product molecule? A A

48. Chemical Rxns 500 - Answer A 2 BCD

49. Chemical Rxns 600 Write a balanced chemical reaction for the following reaction: The combustion of ethane gas, C 2 H 6, produces carbon dioxide gas and water vapor. This reaction is exothermic.

50. Chemical Rxns 600 - Answer 2 C 2 H 6 + 7 O 2  4 CO 2 + 6 H 2 O

51. Stoichiometry 100 What do the coefficients in a chemical reaction mean?

52. Stoichiometry 100 - Answer The coefficients tell us how many of each molecular are involved in the reaction. They also tell us the ratio (in moles) of each compound to the others.

53. Stoichiometry 200 Hydrogen sulfide (H 2 S) burns in air to produce sulfur dioxide and water. How many moles of oxygen gas would be needed to completely burn 8 moles of hydrogen sulfide?

54. Stoichiometry 200 - Answer 12 mol O 2 Equation: 2H 2 S + 3O 2  2SO 2 + 2H 2 O Before: 8 mol xs 0 mol 0 mol Change: -8 mol x(3/2) 12 mol +8 mol +8 mol After: 0 mol xs8 mol 8 mol

55. Stoichiometry 300 What is the ratio of moles of oxygen gas to moles of carbon dioxide in the reaction below? 2C 2 H 6 + 7O 2  4CO 2 + 6H 2 O

56. Stoichiometry 300 - Answer 7 to 4 7:4 7/4

57. Stoichiometry 400 Can you use grams when filling out a BCA table? Why or Why not???

58. Stoichiometry 400 - Answer No grams allowed! Only moles. The ratios in a chemical reaction only apply for moles of each substance.

59. Stoichiometry 500 Calculate the number of moles of sodium oxide that should be produced when 6.50 grams of sodium react with oxygen gas.

60. Stoichiometry 500 - Answer 0.14 mol Na 2 O (6.5g Na)*(1mol/23g Na) = 0.28 mol Na Equation: 4Na + O 2  2Na 2 O Before: 0.28mol xs 0 mol Change: -.28mol -.07mol +0.14mol After: 0 mol xs 0.14 mol

61. Stoichiometry 600 What does stoichimetry help us do?

62. Stoichiometry 600 - Answer ……… Use ratios to determine the amounts of substances that are used up, formed, or produced within a chemical reation.

63. Final Jeopardy

64. Final Jeopardy - Answer