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Drill: Calculate the % composition of each element in MgN 2 O 3

Drill: Calculate the % composition of each element in MgN 2 O 3. CHM II HW. Review PP 06 Work the problems attached to Poly’s website. Molar Conversions. Moles. The standard unit of measure for the amount of a substance in numbers. Dozen. = 12 of anything. Moles.

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Drill: Calculate the % composition of each element in MgN 2 O 3

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  1. Drill: Calculate the % composition of each element in MgN2O3

  2. CHM II HW • Review PP 06 • Work the problems attached to Poly’s website.

  3. Molar Conversions

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

  5. Dozen = 12 of anything

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

  7. Moles = 6.022 x 1023 of anything

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

  9. Moles First

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

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

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

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

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

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

  16. 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

  17. Convert 7.0 g of silicon to moles

  18. Convert 250 g of CaCO3 to moles

  19. Convert 3.0 moles of helium to grams

  20. Convert 11.2 L of oxygen gas at STP to moles

  21. Convert 0.20 moles of helium to volume at STP

  22. Convert: 2.0 x 1024 atoms He to moles

  23. Convert 3.0 moles of glucose to molecules

  24. Convert 250 mL of 0.10 M HCl to moles

  25. Convert 6.8 g NH3 to volume of gas at STP

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

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

  28. Drill: Calculate the number molecules in 32 mg of Fe2O3

  29. First Test • Next Thursday on nomenclature, molar conversions, & reactions.

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

  31. EmpiricalFormula

  32. Lowest whole number ratio of elements in a compound • C6H12O6: EF = CH2O

  33. Determining Empirical formulas from percent composition

  34. Assume 100 g • Change % directly to grams • Use molar conversions to convert grams to moles • Divide each molar amount by the smallest molar amount

  35. Find empirical for a compound with:70.0 % Fe30.0 % O

  36. Find empirical for a compound with:40 % Ca12 % C48 % O

  37. Find empirical for a compound with:40.0 % C6.7 % H53.3 % O

  38. MolecularFormula

  39. The actual whole number for each element in the compound

  40. Molecular FormulaC6H12O6Empirical FormulaCH2O

  41. Solving MF from EF 1) Solve empirical mass 2) Divide EM into MM 3) Multiply EF by quotient

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

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

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

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

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

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

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

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

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