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Unit 6: Chemical Quantities

Unit 6: Chemical Quantities. Chapter 10: Mole and Volume Relationships. The Mole and Volume Relationships. We know that the mass for one mole for different substances will vary because of the molar mass How about volume?. The Mole and Volume Relationships.

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Unit 6: Chemical Quantities

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  1. Unit 6: Chemical Quantities Chapter 10: Mole and Volume Relationships

  2. The Mole and Volume Relationships • We know that the mass for one mole for different substances will vary because of the molar mass • How about volume?

  3. The Mole and Volume Relationships • The volume for a substance will vary because each substance has a different number of atoms in them and each atom is a different size • This is true for liquids and solids • A gas occupies the same amount of space regardless of the size of the atom or molecule

  4. The Mole and Volume Relationships • Avogadro's Hypothesis • Equal volumes of gases at the same temperature and pressure contain equal numbers of particles. • STP • Standard Temperature and Pressure • Temperature is equal to 0˚ C • Pressure is equal to 101.3 kPa or 1 atm • At STP, 1 mol or 6.02 x 1023 representative particles, of any gas occupies a volume of 22.4 L. • 1 mole = 6.02 X 1023 = 22.4 L

  5. The Mole and Volume Relationship • Calculating Volume at STP Volume of gas = Moles of gas X • Practice • Determine the volume in liters of 0.60 mol SO2 gas at STP 22. 4 L 1 mol 0.60 mol SO2 22. 4 L SO2 = 13 L SO3 1 mol SO2

  6. Volume and Molar Mass Relationship • Using Density to find the molar mass of a gas • Cannot find the mass of a gas by weighing it • Remember Density = Mass / Volume or Grams / Liters • Molar mass = density at STP × Molar volume at STP = × Grams mole Grams Liter 22.4 Liters 1 Mole

  7. Volume and Molar Mass Relationship • Example • The density of a gaseous compound containing carbon and oxygen is found to be 1.964 g/L at STP. What is the molar mass of the compound? 1.964 g 22. 4 L = 44.0 g/mol 1 L 1 mol

  8. Mixed Mole Problems Use the map to be able to convert g  atoms, molecules  liters, liters  grams, or any other combination. ALWAYS convert to moles first!

  9. Volume and Molar Mass Relationship • Example • What is the volume, in liters, of 835 g SO3 at STP? • Find out where on the map you are starting (given value) • Convert to moles • Then use the conversion to get where you need to end on the map. • Molar Mass SO3 = 80.1 g/mol 835 g 1 mol 22.4 L = 234 L SO3 80.1 g 1 mol

  10. Volume and Molar Mass Relationship • Example • What is the mass, in grams, of a molecule of aspirin (C9H8O4)? • Molar Mass C9H8O4 = 180.0 g/mol 1 molec 1 mol 180.0 g = 2.99×10-22 g aspirin 6.02×1023 molec 1 mol

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