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MOLE-O!

MOLE-O!. M 1 2 3 4 5 6 7 8 O 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 L 1 2 3 4 5 6 7 8 E 1 2 3 4 5 6 7 8. M–1 Question. If your empirical formula is CH 3 and your molar mass is 45.0 g /mole, what is your molecular formula? Answer. M-2 Question.

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MOLE-O!

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  1. MOLE-O!

  2. M • 12345678 • O • 12345678 • 910111213141516 • L • 12345678 • E • 12345678

  3. M–1 Question • If your empirical formula is CH3 and your molar mass is 45.0 g/mole, what is your molecular formula? • Answer

  4. M-2 Question • If your empirical formula is CH2 and your molar mass is 28.0 g/mole, what is your molecular formula? • Answer

  5. M-3 Question • If your empirical formula is CH2O and your molar mass is 360.0 g/mole, what is your molecular formula? • Answer

  6. M-4 Question • If your empirical formula is CH3 and your molar mass is 60.0 g/mole, what is your molecular formula? • Answer

  7. M-5 Question • If your empirical formula is CH2 and your molar mass is 42.0 g/mole, what is your molecular formula? • Answer

  8. M-6 Question • If your empirical formula is CH2O and your molar mass is 180.0 g/mole, what is your molecular formula? • Answer

  9. M-7 Question • If your empirical formula is CH3 and your molar mass is 30.0 g/mole, what is your molecular formula? • Answer

  10. M-8 Question • If your empirical formula is CH2O and your molar mass is 90.0 g/mole, what is your molecular formula? • Answer

  11. O-1 Question • What is the volume (in L) of 52.0 grams of NH3 at STP? • Answer

  12. O-2 Question • How many formula units are contained in 0.285 grams of potassium hydroxide? • Answer

  13. O-3 Question • You have 8.3 X 108 atoms of zinc. How many moles is this? • Answer

  14. O-4 Question • What is the molar mass of calcium nitrate? • Answer

  15. O-5 Question • What is the molar mass of copper (II) nitrate? • Answer

  16. O-6 Question • You have 264 grams of sodium hydroxide. How many moles is this? • Answer

  17. O-7 Question • You have 1.2 grams of sodium. How many atoms is this? • Answer

  18. O-8 Question • What is the volume (in L) of 4,260 atoms of Neon at STP? • Answer

  19. O-9 Question • What is the volume (in L) of 0.847 grams of carbon dioxide at STP? • Answer

  20. O-10 Question • What is the mass (in grams) of 0.035 moles of chromium (II) chloride? • Answer

  21. O-11 Question • What is the mass (in grams) of 1.74 X 1016 formula units of sodium hydroxide? • Answer

  22. O-12 Question • How many molecules are contained in 26 grams of water? • Answer

  23. O-13 Question • What is the mass of 3 atoms of helium? • Answer

  24. O-14 Question • What is the volume (in L) of 56.27 grams of nitrogen dioxide at STP? • Answer

  25. O-15 Question • What is the mass of 3,720 molecules of O2 gas? • Answer

  26. O-16 Question • What is the mass (in grams) of 263 L of dinitrogenpentoxide at STP? • Answer

  27. L-1 Question • A 1.023 gram sample of hydrated copper (II) sulfate, CuSO4• X H2O, is heated to remove all the water and produce 0.653 grams of the anhydrous salt. What is the value of “X?” Answer

  28. L-2 Question • What is the percent water in copper (II) nitrate trihydrate? • Answer

  29. L-3 Question • What is the percent water in nickel (II) chloride hexahydrate? • Answer

  30. L-4 Question • Hydrated calcium sulfate, CaSO4• X H2O, contains 20.93% water. What is the value of “X?” • Answer

  31. L-5 Question • Borax powder has the formula Na2B4O7• X H2O. When 2.145 grams of the hydrate are heated and the water is removed, 1.130 grams of anhydrous salt remain. What is the value of “X?” Answer

  32. L-6 Question • What is the percent water in magnesium nitrate hexahydrate? • Answer

  33. L-7 Question • What is the percent water in barium chloride dihydrate? • Answer

  34. L-8 Question • If 1.687 grams of epsom salt, MgSO4• X H2O, is heat to remove all water, 0.824 grams of salt remain. What is the value of “X?” • Answer

  35. E-1 Question • What is the percent lead in lead (II) chloride? • Answer

  36. E-2 Question • What is the percent potassium in potassium dichromate? • Answer

  37. E-3 Question • What is the empirical formula of a compound composed of 77.7% iron and 22.3% oxygen? • Answer

  38. E-4 Question • What is the empirical formula of a compound composed of 44.0% iron and 56.0% chlorine? • Answer

  39. E-5 Question • What is the empirical formula of a compound composed of 34.4% iron and 65.6% chlorine? • Answer

  40. E-6 Question • What is the percent sulfur in iron (II) sulfide? • Answer

  41. E-7 Question • What is the percent sodium in sodium sulfate? • Answer

  42. E-8 Question • What is the empirical formula of a compound composed of 69.9% iron and 30.1% oxygen? • Answer

  43. M-1 Answer • C3H9

  44. M-2 Answer • C2H4

  45. M-3 Answer • C12H24O12

  46. M-4 Answer • C4H12

  47. M-5 Answer • C3H6

  48. M-6 Answer • C6H12O6

  49. M-7 Answer • C2H6

  50. M-8 Answer • C3H6O3

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