Conversion Factors 1. Write out conversion factors between the moles of each element and the moles of the compound C 5 H 12 . 2. Write out conversion factors between the moles of each element and the moles of the compound C 27 H 46 O. 3. Write out conversion factors between the moles of each element and the moles of the compound C 6 H 12 O 6 . 4. Write out the conversion factor of the given element in the given compound using the mass percent composition. a) Carbon dioxide is 27.19% carbon by mass b) Butane is 17.34% hydrogen by mass c) C 6 H 8 O 7 is 58.29% oxygen by mass 5. Write out the conversion factor of the given element in the given compound using the mass percent composition. a) Ethanol is 13.13% hydrogen by mass b) Aluminum nitrate is 19.73% nitrogen by mass c) Methyl butanoate is 58.8% carbon by mass 6. Write out the conversion factor of the given element in the given compound using the mass percent composition. a) Propane is 81.68% carbon by mass b) Ethylene is 14.14% hydrogen by mass c) Aluminum oxide is 52.9% aluminum by mass The Mole Concept 7. How many moles of atoms are in the following? a) 8.22 x 10 24 As atoms b) 4.41 x 10 22 Ne atoms c) 6.77 x 10 23 Li atoms d) 2.10 x 10 21 S atoms 8. How many atoms are in the following given numbers of moles of an element? a) 0.994 mol F b) 4.39 mol Sr c) 9.1 x 10 -3 mol B d) 13.8 mol Cl 9. How many moles of atoms are in the following? a) 2.13 x 10 25 He atoms b) 3.65 x 10 22 Ga atoms c) 6.022 x 10 23 Mg atoms d) 1.04 x 10 24 Cu atoms 10. Complete the table: 0 1 2 Element Moles Number of Atoms Se 0.0112 NaN K NaN 1.55 x 1023 Ti 2.34 NaN Br NaN 7.12 x 1022 11. Complete the table: 0 1 2 Element Moles Number of Atoms P 13.2 NaN Au 0.222 NaN F NaN 5.02 x 1024 Be NaN 1.98 x 1023 12. Complete the table: 0 1 2 Element Moles Number of Atoms O NaN 9.54 x 1021 Zr 1.30 x 10-6 NaN Bk 25.3 NaN Ba NaN 7.71 x 1024 13. Complete the table: 0 1 2 Element Moles Mass N NaN 75.4g W NaN 13.9g Ge 0.00784 NaN Rb 4.09 NaN 14. Complete the table: 0 1 2 Element Moles Mass Co NaN 62.4g Hg 2.23 x 10-4 NaN Te 18.6 NaN Al NaN 4.97g 15. Complete the table: 0 1 2 Element Moles Mass Li 244 NaN Y 0.653 NaN B NaN 20.7g He NaN 0.00422g 16. Calculate the mass in grams of the following: a) 4.45 x 10 19 Ag atoms b) 5.50 x 10 24 Bi atoms c) 2.08 x 10 21 Se atoms d) 7.31 x 10 24 Ar atoms 17. Calculate the number of atoms in each of the following: a) 14.8g Al b) 3.98g Ca c) 1.90g Co d) 26.7g S 18. Calculate the mass of the following: a) 3.72 x 10 20 Cd atoms b) 6.01 x 10 23 Sb atoms c) 9.43 x 10 26 F atoms d) 2.84 x 10 22 Re atoms 19. Complete the table: 0 1 2 3 Element Mass Moles Number of Atoms Sn NaN 3.65 NaN Xe NaN 0.0983 NaN H 65.5mg NaN NaN Si NaN NaN 4.35 x 1024 20. Complete the table: 0 1 2 3 Element Mass Moles Number of Atoms Ca NaN NaN 6.18 x 1021 Br 0.138kg NaN NaN Ga NaN NaN 9.29 x 1023 K NaN 10.4 NaN 21. Complete the table: 0 1 2 3 Element Mass Moles Number of Atoms Be 226mg NaN NaN S NaN NaN 7.36 x 1020 Nb NaN 0.104 NaN N 0.00391kg NaN NaN 22. Calculate the mass of the following in grams: a) 6.10 mol carbon monoxide b) 0.364 mol sulfur hexafluoride c) 4.44 mol potassium hydroxide d) 1.71 mol lithium nitrate 23. Calculate the mass of the following in grams: a) 13.4 mol sodium chloride b) 0.223 kmol nitrogen dioxide c) 0.00322 mol boron tribromide d) 144 mmol xenon tetroxide 24. Calculate the number of moles of molecules for the following: a) 29.8g ammonium iodide b) 8.34g potassium cyanide c) 3.50mg sodium sulfate d) 0.0888kg hydrochloric acid 25. Complete the table: 0 1 2 3 Compound Mass Moles Number of Molecules H2SO4 188kg NaN NaN NaBr NaN 0.318 NaN KClO3 4.05mg NaN NaN NH3 NaN 7.10 NaN 26. Complete the table: 0 1 2 3 Compound Mass Moles Number of Molecules NO NaN 0.929 NaN CCl4 0.133kg NaN NaN HF 16.9g NaN NaN CS2 NaN 0.00268 NaN 27. Complete the table: 0 1 2 3 Compound Mass Moles Number of Molecules CH4 NaN 3.45 NaN NaOH 42.2mg NaN NaN LiCl NaN 0.00215 NaN AgNO3 311g NaN NaN 28. Calculate the mass of the following in grams: a) 3.19 x 10 24 SrCl 2 formula units b) 2.81 x 10 21 Na 3 PO 4 formula units c) 7.70 x 10 22 KBrO 3 formula units d) 4.51 x 10 19 HNO 3 formula units 29. Calculate the mass of the following in grams: a) 4.30 x 10 23 KCN formula units b) 6.25 x 10 25 FeCl 3 formula units c) 9.64 x 10 22 HF molecules d) 7.38 x 10 18 CO 2 molecules 30. Calculate the number of molecules of the following: a) 13.2g SO 2 b) 9.03g CH 4 c) 0.00888g H 2 d) 157g LiBr 31. A sample of CuS has a mass of 0.67mg. Calculate the number of formula units. 32. A sample of VF 4 has a mass of 0.0076kg. Calculate the number of formula units. 33. A sample of C 6 H 6 has a mass of 15ng. Calculate the number of molecules. Chemical Formulas as Conversion Factors 34. Calculate the number of moles of O in the following: a) 11.4 mol CO 2 b) 0.761 mol H 2 O c) 4.08 mol N 2 O 5 d) 0.302 mol HNO 3 35. Calculate the number of moles of H in the following: a) 1.44 mol H 2 SO 4 b) 0.00373 mol C 3 H 8 c) 22.4 mol HNO 2 d) 0.0200 mol C 3 H 9 N 36. How many moles of H are in 1.85 mol [Cr(OH 2 ) 5 Cl] Cl•H 2 O? 37. Calculate the mass in kg of the following which each contain 3.5 x 10 2 kg of lithium. a) Li 2 SO 4 b) LiOH c) LiBr 38. Calculate the mass in mg of the following which each contain 2.2 x 10 4 mg of silver. a) Ag 2 O b) AgI c) Ag 3 N 39. Calculate the mass in kg of the following which each contain 7.1 x 10 2 kg of sodium. a) NaCl b) Na 2 CO 3 c) Na 3 PO 4 40. Which of the following contains the greatest number of moles of oxygen? Show all work. a) 3.03 mol C 2 H 6 O 2 b) 16.9 mol N 2 O 3 c) 8.27 mol Sr(NO 3 ) 2 d) 0.0180 mol BaSO 4 41. Which of the following contains the greatest number of moles of hydrogen? a) 0.712 mol C 3 H 6 O 3 b) 2.40 mol H 2 O c) 3.49 mol C 4 H 10 d) 7.48 mol NH 4 OH 42. Of the following compounds containing the ammonium ion, which contains the greatest number of moles of nitrogen? Show all work. a) 11.4 mol NH 4 NO 3 b) 9.65 mol (NH 4 ) 2 O c) 83.4 mol NH 4 I d) 0.997 mol (NH 4 ) 3 PO 4 Mass Percent Composition 43. An 8.91g sample of an organic compound is found to contain 3.34g C, 0.98g H, 2.61g O, and 1.98g N. Determine the mass percent of each element. 44. BaSO 4 is approximately 58.84% barium by mass. Calculate the mass of barium in grams in a 7.22g sample of BaSO 4 . 45. Calculate the mass percent composition of oxygen in the following compounds. a) CrO 3 b) SO 2 c) NaOH d) Al 2 (SO 4 ) 3 46. Calculate the mass percent composition of all the individual elements in each of the following compounds. a) SrCl 2 b) Fe 2 O 3 c) CsF d) NaCN 47. Calculate the mass percent composition of all the individual elements in each of the following compounds. a) HClO 3 b) AgBr c) PbSO 4 d) CH 4 48. Calculate the mass percent composition of all the individual elements in each of the following compounds. a) Be 3 N 2 b) IF 7 c) ZnF 2 d) Ca(OH) 2 Calculating Empirical Formulas 49. An organic compound is found to have 36.03g of carbon, 6.048g hydrogen, and 16.00g oxygen. Determine the empirical formula of the organic compound. 50. An organic compound is found to have 32.07g of carbon, 3.36g of hydrogen, 18.63g of nitrogen, and 10.72g of oxygen. Determine the empirical formula of the organic compound. 51. An organic compound is found to have 15.97g of carbon, 2.016g of hydrogen, and 21.28g of oxygen. Determine the empirical formula of the organic compound. 52. The nonsteroidal anti-inflammatory drug Ibuprofen consists of 75.69% carbon, 8.80% hydrogen, and 15.51% oxygen. Determine the empirical formula of ibuprofen. 53. The chemical compound cinnamaldehyde is what gives cinnamon its flavor and odor. When tested in a lab, it is found to consist of 81.79% carbon, 6.10% hydrogen, and 12.11% oxygen. Determine the empirical formula of cinnamaldehyde. 54. The antiviral drug zanamivir is used in influenza vaccinations. It consists of 43.37% carbon, 6.07% hydrogen, 16.86% nitrogen, and 33.70% oxygen. Determine the empirical formula of zanamivir. Calculating Molecular Formulas 55. Determine the molecular formula of each of the following using the given empirical formulas and total molar masses. a) CO 2 H, 225.09g/mol b) CClN, 184.41g/mol c) C 2 H 3 O, 86.09g/mol d) C 4 H 8 O, 144.21g/mol 56. Determine the molecular formula of each of the following using the given empirical formulas and total molar masses. a) C 5 H 8 , 136.23 g/mol b) CH 3 O 4 P, 660.02 g/mol c) C 2 H 5 N, 86.14g/mol d) CH, 78.11g/mol 57. Determine the molecular formula of each of the following using the given empirical formulas and total molar masses. a) C 6 H 8 O, 288.37g/mol b) CH 2 N 2 O 2 , 296.18g/mol c) C 2 H 7 NS, 77.16g/mol d) C 11 H 22 O, 340.57g/mol Challenge Problems 58. How many ethanol molecules are in a 613mL container of pure ethanol? Ethanol has a density of 0.7893 g/cm 3 . 59. Complete the table: 0 1 2 3 Substance Mass Moles Number of Particles CdF2 NaN 0.0389 NaN N 17.3mg NaN NaN Ag 1.02kg NaN NaN HNO3 NaN NaN 4.55 x 1021 60. Complete the table: 0 1 2 3 4 5 Formula Name Mass %Na %Cl %O NaClO2 NaN NaN NaN NaN NaN NaClO3 NaN NaN NaN NaN NaN NaClO4 NaN NaN NaN NaN NaN 61. Aldrin is an insecticide that was commonly used in soil fields until it was banned in many countries. It is found to consist of 39.50% carbon, 2.21% hydrogen, and 58.29% chlorine. Its molar mass is 364.884g/mol. Using this information, determine the molecular formula of Aldrin. 62. A solution contains approximately 45.4% KBr by mass within it. The solution has a density of 2.21g/mL. What volume of the solution contains 2.0g of potassium? 63. A sample of an acid is analyzed in a laboratory and is found to consist of 40.00% C, 6.71% H, and 53.29% O. Its molar mass is 90.078g/mol. Determine the acid’s molecular compound. Search the formula in your text or an internet source and write its name.