2. Quantities in Chemical Reactions Review

3. Definitions $100 $200 $300 $400 $500 Quantities Balanced Chemical Equations Additional Calculations Team 1Team 2Team 3Team 4 $200 Moles & Mass Empirical Formulas

4. Definitions: $100 Answer A unit of measurement expressing amount of a species

5. Definitions: $100 Mole Return to Main

6. Definitions: $200 Answer The relationship between amounts of species in a reaction

7. Definitions: $200 Return to Main Stoichiometry

8. Definitions: $300 Answer The mass of one mole of a particular chemical species

9. Definitions: $300 Return to Main Atomic Mass

10. Definitions: $400 Answer 1 mole of any gas occupies 22.4 L

11. Definitions: $400 Return to Main STP

12. Definitions: $500 Answer The number of particles in one mole of a species

13. Definitions: $500 Return to Main Avogadro’s Number

14. Moles & Mass: $100 Answer Molar mass of (NH­ 4 ) 2 SO 4

15. Moles & Mass: $100 Return to Main 132.14 g/mol

16. Moles & Mass: $200 Answer Number of atoms in 0.00511 mol of NaNO 3

17. Moles & Mass: $200 Return to Main 1.539 * 10 23 atoms

18. Moles & Mass: $300 Answer Number of grams in 2.3 x 10 -4 moles of calcium phosphate, Ca 3 (PO 3 ) 2 ?

19. Moles & Mass: $300 Return to Main 0.116 grams

20. Scores Proceed

21. Moles & Mass: $400 Answer Using your knowledge of mole calculations and unit conversions, determine how many atoms there are in 1 gallon of gasoline. Assume that the molecular formula for gasoline is C 6 H 14 and that the density of gasoline is approximately 0.85 grams/mL. Note: there are 3785 mL per gallon.

22. Moles & Mass: $400 Return to Main 5.29067 * 10 23 atoms

23. Moles & Mass: $500 Answer Number of molecules are there in 450 grams of Na 2 SO 4

24. Moles & Mass: $500 Return to Main 1.91 * 10 24 molecules

25. Quantities: $100 Answer CH 4 + 3 O 2  CO 2 + 2 H 2 Moles of CO 2 produced if 26 g of CH 4 is burned

26. Quantities: $100 Return to Main 16 moles

27. Quantities: $200 Answer CH 4 + 3 O 2  CO 2 + 2 H 2 Moles of CO 2 produced if 67.2 L of CH 4 is burned

28. Quantities: $200 Return to Main 3 moles

29. Quantities: $300 Answer CaCO 3(s)  CO 2(g) + CaO (s) How many grams of calcium carbonate would you need to make 3.45 L of carbon dioxide (assume STP)?

30. Quantities: $300 Return to Main 100/6 moles

31. Quantities: $400 Answer H 2 gas can be produced by reacting CH 4 with high temperature steam. How many particles of H 2 are produced when 158 g of CH 4 reacts with steam? CH 4(g) + H 2 O (g) → CO (g) + 3 H 2(g)

32. Quantities: $400 Return to Main 180 * 10 23 = 1.8 * 10 25

33. Quantities: $500 Answer The Haber process combines hydrogen (H 2 ) with nitrogen (N 2 ) to produce ammonia (NH 3 ). At STP, how many moles of ammonia can you produce, given that you have 44.8 L of H 2 ? N 2 ­ (g) +3H 2(g) → 2NH 3(g)

34. Quantities: $500 Return to Main 1.333 moles

35. Formulas: $100 Answer The empirical formulas, given the % composition for respective elements: Fe = 63.53%, S = 36.47% The empirical formulas, given the % composition for respective elements: Fe = 63.53%, S = 36.47%

36. Formulas: $100 Return to Main FeS

37. Formulas: $200 Answer The empirical formulas, given the % composition for respective elements: Na = 21.6%, Cl = 33.3%, O = 45.1% The empirical formulas, given the % composition for respective elements: Na = 21.6%, Cl = 33.3%, O = 45.1%

38. Formulas: $200 Return to Main NaClO 3

39. Formulas: $300 Answer The empirical formulas, given the % composition for respective elements: Cr = 26.52%, S = 24.52%, O = 48.96% The empirical formulas, given the % composition for respective elements: Cr = 26.52%, S = 24.52%, O = 48.96%

40. Formulas: $300 Return to Main CrS 3 O 6

41. Formulas: $400 Answer A compound of unknown identity is made up of 40.1% sulfur and 59.9% oxygen (by mass).

42. Formulas: $400 Return to Main SO 3

43. Formulas : $500 Answer The empirical formulas, given the % composition for respective elements: C = 63.1%, H = 11.92%, F = 24.97% The empirical formulas, given the % composition for respective elements: C = 63.1%, H = 11.92%, F = 24.97%

44. Formulas: $500 Return to Main C 5 H 12 F

45. Balanced Chemical Equations: $100 Answer __CHCl 3 + __Cl 2 → __CCl 4 + __HCl

46. Balanced Chemical Equations: $100 Return to Main Already balanced CHCl 3 + Cl 2 → CCl 4 + HCl Already balanced CHCl 3 + Cl 2 → CCl 4 + HCl

47. Balanced Chemical Equations: $200 Answer __SnO 2 + __H 2 → __Sn + __H 2 O

48. Balanced Chemical Equations: $200 Return to Main SnO 2 + 2H 2 → Sn + 2H 2 O

49. Balanced Chemical Equations: $300 Answer __KOH + __H 3 PO 4 →__K 3 PO 4 + __H 2 O

50. Balanced Chemical Equations: $300 Return to Main 3 KOH + H 3 PO 4 → K 3 PO 4 + 3 H 2 O

51. Balanced Chemical Equations: $400 Answer __KNO 3 + __H 2 CO 3 →__K 2 CO 3 + __HNO 3

52. Balanced Chemical Equations: $400 Return to Main 2 KNO 3 + H 2 CO 3 → K 2 CO 3 + 2 HNO 3

53. Balanced Chemical Equations: $500 Answer __ CaCl 2 + __ Na 3 PO 4 → __ Ca 3 (PO 4 ) 2 + __ NaCl __ CaCl 2 + __ Na 3 PO 4 → __ Ca 3 (PO 4 ) 2 + __ NaCl

54. Balanced Chemical Equations: $500 Return to Main 3 CaCl 2 + 2 Na 3 PO 4 → Ca 3 (PO 4 ) 2 + 6 NaCl 3 CaCl 2 + 2 Na 3 PO 4 → Ca 3 (PO 4 ) 2 + 6 NaCl

55. Additional Calculations: $100 Answer How many grams of H 2 are produced if there are 18 grams of H 2 O? CH 4(g) + H 2 O (g) → CO (g) + 3 H 2(g) How many grams of H 2 are produced if there are 18 grams of H 2 O? CH 4(g) + H 2 O (g) → CO (g) + 3 H 2(g)

56. Additional Calculations: $100 Return to Main 3 grams

57. Additional Calculations: $200 Answer Na 2 S(aq) + AgNO 3 (aq) → Ag 2 S(s) + NaNO 3 (aq) How many grams of Ag 2 S can be produced from 7.88 grams of AgNO 3 and excess Na 2 S?

58. Additional Calculations: $200 Return to Main 5.74 grams

59. Additional Calculations: $300 Answer CuSO 4 + Zn → ZnSO 4 + Cu How many grams of copper are produced from 2.9 grams of zinc consumed with excess CuSO 4 in this reaction?

60. Additional Calculations: $300 Return to Main 2.8 grams

61. Additional Calculations: $400 Answer Limiting reagent when there is 8 grams of CH 4 and 18 grams of H 2 O CH 4(g) + H 2 O (g) → CO (g) + 3 H 2(g) Limiting reagent when there is 8 grams of CH 4 and 18 grams of H 2 O CH 4(g) + H 2 O (g) → CO (g) + 3 H 2(g)

62. Additional Calculations: $400 Return to Main CH 4(g)

63. Additional Calculations: $500 Answer 4.00 g of the gas was produced in a flask containing 24.8 g of the reactant. Determine the percent yield of the student's reaction.

64. Additional Calculations: $500 Return to Main 30.3%

65. Titration Calculation Proceed

66. Answer 3 NH 4 NO 3 + Na 3 PO 4  (NH 4 ) 3 PO 4 + 3 NaNO 3 a)With 30 g of NH 4 NO 3 and 50 g of Na 3 PO 4, identify the limiting reagent. b) What is the maximum amount of each product that can be formed? 3 NH 4 NO 3 + Na 3 PO 4  (NH 4 ) 3 PO 4 + 3 NaNO 3 a)With 30 g of NH 4 NO 3 and 50 g of Na 3 PO 4, identify the limiting reagent. b) What is the maximum amount of each product that can be formed?

67. Return to Main NH 4 NO 3