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Drill: Calculate the % composition of each element in Fe 2 (SO 4 ) 3

Drill: Calculate the % composition of each element in Fe 2 (SO 4 ) 3. Molar Conversions. Moles. The standard unit of measure for the amount of a substance in numbers. Dozen. = 12 of anything. Moles. = the amount of a substance that would = its mass in g from the PT. Moles.

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Drill: Calculate the % composition of each element in Fe 2 (SO 4 ) 3

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  1. Drill: Calculate the % composition of each element in Fe2(SO4)3

  2. Molar Conversions

  3. Moles • The standard unit of measure for the amount of a substance in numbers

  4. Dozen = 12 of anything

  5. Moles = the amount of a substance that would = its mass in g from the PT

  6. Moles = 6.022 x 1023 of anything

  7. Molar Conversions • Mass to moles • Volume of a gas to moles • Particles to moles • Volume of a solution to moles

  8. Moles First

  9. Mass to Moles • Use atomic masses from the periodic table • NaCl = 58.5 g/mole

  10. Gas Volume to Moles • At STP: 22.4 L/mole • Non-STP: PV = nRT PV RT n =

  11. Particles to Moles • Use Avogadro’s Number • 6.02 x 1023 atoms, molecules, etc/mole

  12. Soln Volume to Moles • Multiply molarity times volume • n = M x V

  13. Solution Measures • Molarity (M) = the number of moles of solute per liter of solution • Others later

  14. Calculate the atomic mass of the element made up of the following isotopes:99.50 % H-10.30 % H-20.20 % H-3

  15. Calculate the atomic mass of the element made up of the following isotopes:5.0 % Pu-242, 5.0 % Pu-24380.0 % Pu-244, & 10.0 % Pu-245

  16. Convert 7.0 g of silicon to moles

  17. Convert 250 g of CaCO3 to moles

  18. Convert 3.0 moles of helium to grams

  19. Convert 5.6 L of oxygen gas at STP to moles

  20. Convert 0.50 moles of helium to volume at STP

  21. Convert: 2.0 x 1024 atoms He to moles

  22. Convert 3.0 moles of glucose to molecules

  23. Convert 250 mL of 0.10 M HCl to moles

  24. Drill: Determine the volume required to make 60.0 g NaOH into a 0.75 M solution

  25. Convert 6.8 g NH3 to volume at STP

  26. Convert 3.0 x 1025 molecules of CO2 to mass in kg

  27. Calculate the number of oxygen atoms in 32 mg of Fe2O3

  28. Calculate the number of atoms in 16 ng of Fe2(SO4)3

  29. Drill: Calculate the mass of solute required to make 40.0 mL of0.25 M Pb(NO3)2

  30. Test Review on Nomenclature, Molar conversions, & % Composition.

  31. Calculate the % composition of each element in Pb(NO3)2

  32. Calculate the empirical formula of a substance comtaining 62.7 % Po, 28.8 % O, & 8.4 % N.

  33. Calculate the molecular formula of a substance with an empirical formula of NH2 & a molecular mass of 32 g/mole.

  34. Name each of the following: • SeO MgS • PbO2 Cl2O • KNO3 ScCl3

  35. Derive formulas for each: • Cesium oxide • Barium chloride • Calcium phosphate • Manganese(II) chlorate

  36. Name each of the following: NH4Cl BaSO4 KC2H3O2 K2HPO3 KNO3 CuBrO Li2CO3 MgC2O4

  37. Name each of the following: HCl H2SO4 H2S H3PO3 HNO3 HBrO H2CO3 HBrO4

  38. Calculate the number of hydrogen atoms in 1.8 kg of PH5.

  39. Calculate the volume at STP of 6.0 ng of NO.

  40. Calculate the mass of KBr required to make 250 mL of a 0.40 M solution.

  41. Chapter 3 General • Define all the Key Terms on page 74

  42. Atomic Mass • Work problems: • 1 - 9 • on page 75

  43. Avogadro’s Num. • Work problems: • 11 - 18 • on page 75

  44. Molar Conversions • Work problems: • 18 - 26 • on page 75 & 76

  45. % Composition • Work problems: • 27 - 34 • on page 76

  46. Empirical Formula • Work problems: • 35 - 46 • on page 76 & 77

  47. Balancing Rxns • Work problems: • 49 & 54 • on page 77

  48. Stoichiometry • Work problems: • 55 & 64 • on page 77 & 78

  49. Limiting Reactant • Work problems: • 65 & 74 • on page 78 & 79

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