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5. stoichmixturesAcids/bases 10 Point 20 Points 30 Points 40 Points 50 Points 10 Point 20 Points 30 Points 40 Points 50 Points 30 Points 40 Points 50 Points gasesreactions

6. Balance the following reaction: AlBr 3 + K 2 SO 4  KBr + Al 2 (SO 4 ) 3

7. 2AlBr 3 + 3K 2 SO 4  6KBr + Al 2 (SO 4 ) 3

8. What type of reaction is this: N 2 + 3H 2  2 NH 3

9. synthesis

10. Write and balance the following reaction: Sodium phosphate reacts with cobalt (II) carbonate to form cobalt (II) phosphate and sodium carbonate

11. 2Na 3 PO 4 +3 CoCO 3  3 Na 2 CO 3 + Co 3 (PO 4 ) 2

12. Write/balance the following equation and predict the products: Sodium fluoride reacts with bromine

13. 2 NaF + Br 2  NR

14. Write the net ionic reaction for: 2NaCl(aq)+Pb(NO 3 ) 2 (aq)  PbCl 2 (s)+2NaNO 3 (aq)

15. 2Cl - (aq)+Pb 2+ (aq)  PbCl 2 (s)

16. What is the molecular formula of the following: A compound with an empirical formula of CFBrO and a molar mass of 254.7 grams per mole.

17. C 2 F 2 Br 2 O 2

18. Convert 3.5 g of oxygen to molecules.

19. 6.59 x 10 22

20. How many moles of N2 will be produced if 3.5 moles of O2 react? ___NH3 + ___O2  ___N2 + ___H2O

21. 2.33 mol

22. Given the following reaction: potassium reacts with water to produce potassium hydroxide and hydrogen How many grams of hydrogen will be formed from the reaction of 2.89 g of water?

23. 0.16 g hydrogen

24. Given the following equation: P 4 + O 2  P 4 O 10 If I react 2.04 g of phosphorus with 5.78 g of oxygen, how much product will be produced in grams?

25. 4.67 g

26. The pressure of air in a 2.25 L container is 1.2 atm. What is the new pressure if the air is transferred to a 6.5 L container?

27. 0.42 L

28. A gas has a volume of 345 mL at a pressure of 2.3 atm and a temperature of 29°C. If the pressure changes to 89 kPa and the temperature increase to 50°C, what is the new volume of the gas?

29. 964 mL

30. What is the volume of 4.67 mol of nitrogen gas at STP?

31. 104.6 L

32. If air has an average molar mass of 29 g/mol, what is the density of air at 25°C and 770 mmHg?

33. 1.2 g/L

34. Given the following reaction: NH 3 + NO  N 2 + H 2 O How many grams of ammonia are needed to produce 2.45 L of nitrogen at 30°C and 1.5 atm?

35. 2.04 g

36. If 50 mL of pure acetone is mixed with 0.450 L of water, what is the percent by volume of acetone?

37. 10%

38. Calculate the mass of sodium hydroxide required to prepare a 5.78 M solution dissolved in 3400 mL of solution.

39. 786 g

40. What is the molality of 23 g of copper (II) carbonate dissolved in 67 g of water?

41. 2.84 m

42. If I have 40 g of ammonium chloride in 100 g of water at 70°C, how many grams of solute do I need to add to make the solution saturated?

43. 20 g

44. What is the new boiling point of 130 g of water with 24 g of magnesium chloride dissolved in the water?

45. 103.07 degrees celsius

46. HNO 3 Acid or base?

47. acid

48. What is the pH of 0.345 M HCl?

49. 0.46

50. What is the pH of 0.23 M NaOH?

51. 13.36

52. Ca(OH) 2 + H 2 SO 4  Predict products and balance

53. Ca(OH) 2 + H 2 SO 4  CaSO 4 +2 H 2 O

54. What is the molarity of a HNO3 solution if 43.33 mL of 0.1000 M KOH solution is needed to neutralize 20 mL of the acid solution?

55. 0.22 M

56. Make your wager

57. A gaseous compound is 25% carbon, 2.1% hydrogen, and 73% chlorine. At 100 o C, its density at 99.97 kPa is 3.12 x 10 -3 g/mL. What is the molecular formula of this compound?

58. C2H2Cl2