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Section 3: Moles of Compounds

Section 3: Moles of Compounds. Chemical Composition. Learning Goals. Recognize the mole relationships shown by a chemical formula. Calculate the molar mass of a compound. Convert between the number of moles and mass of a compound.

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Section 3: Moles of Compounds

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  1. Section 3: Moles of Compounds Chemical Composition

  2. Learning Goals • Recognize the mole relationships shown by a chemical formula. • Calculate the molar mass of a compound. • Convert between the number of moles and mass of a compound. • Apply conversion factors to determine the number of atoms or ions in a known mass of a compound.

  3. Chemical Formulas and the Mole • Chemical formulas indicate the numbers and types of atoms contained in one unit of the compound.

  4. Chemical Formulas and the Mole • One mole of CCl2F2 contains one mole of C atoms, two moles of Cl atoms, and two moles of F atoms.

  5. Practice • Determine the number of moles of Cl- ions in 2.50 mol of zinc chloride.

  6. Practice • How many moles of oxygen atoms are present in 5.00 mol of diphosphoruspentoxide?

  7. The Molar Mass of Compounds • The molar mass of a compound equals the molar mass of each element, multiplied by the moles of that element in the chemical formula, added together. • The molar mass of a compound demonstrates the law of conservation of mass.

  8. Practice • Determine the molar mass of hydrogen cyanide.

  9. Practice • Determine the molar mass of calcium chloride.

  10. Converting Moles to Mass • For elements, the conversion factor is the molar mass of the compound. • The procedure is the same for compounds, except that you must first calculate the molar mass of the compound.

  11. Practice • What is the mass of 3.25 mol of sulfuric acid?

  12. Converting Mass to Moles • The conversion factor is the inverse of the molar mass of the compound.

  13. Practice • Determine the number of moles present in 35.0 g of hydrochloric acid.

  14. Converting Mass to Particles • Convert mass to moles of compound with the inverse of molar mass. • Convert moles to particles with Avogadro’s number.

  15. Practice • A sample of sodium sulfite has a mass of 2.25 g. • How many sodium ions are present? • How many sulfite ions are present? • What is the mass in grams of one formula unit of sodium sulfite?

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