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The Mole–Mass Relationship

10.2. The Mole–Mass Relationship. The Mole–Mass Relationship How do you convert the mass of a substance to the number of moles of the substance?. 10.2. The Mole–Mass Relationship.

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The Mole–Mass Relationship

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  1. 10.2 The Mole–Mass Relationship • The Mole–Mass Relationship • How do you convert the mass of a substance to the number of moles of the substance?

  2. 10.2 The Mole–Mass Relationship • Use the molar mass of an element or compound to convert between the mass of a substance and the moles of a substance.

  3. 10.5

  4. for Sample Problem 10.5

  5. 10.6

  6. for Sample Problem 10.6

  7. 10.2 The Mole–Volume Relationship • The Mole–Volume Relationship • What is the volume of a gas at STP?

  8. 10.2 The Mole–Volume Relationship • Avogadro’s hypothesis states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.

  9. 10.2 The Mole–Volume Relationship • The volume of a gas varies with temperature and pressure. Because of these variations, the volume of a gas is usually measured at a standard temperature and pressure. • Standard temperature and pressure (STP) means a temperature of 0°C and a pressure of 101.3 kPa, or 1 atmosphere (atm).

  10. 10.2 The Mole–Volume Relationship • At STP, 1 mol or, 6.02  1023 representative particles, of any gas occupies a volume of 22.4 L. • The quantity 22.4 L is called the molar volume of a gas.

  11. 10.2 The Mole–Volume Relationship • Calculating Volume at STP

  12. 10.7

  13. for Sample Problem 10.7

  14. 10.2 The Mole–Volume Relationship • Calculating Molar Mass from Density

  15. 10.8

  16. for Sample Problem 10.8

  17. 10.2 The Mole Road Map

  18. 10.2 The Mole Road Map

  19. 10.2 The Mole Road Map

  20. 10.2 The Mole Road Map • The Mole Road Map

  21. 10.2 Section Quiz. • 1. Calculate the mass in grams of a sample containing 1.85 x 1034 molecules of water. • 3.07 x 1010 g • 5.53 x 1011 g • 188 g • 8.46 x 103 g

  22. 10.2 Section Quiz. • 2. Calculate the number of moles in a spoonful of table sugar (C12H22O11) having a mass of 10.5 g. • 32.6 mol • 3.59  103 mol • 3.07  10–3 mol • 1.85  1022 mol

  23. 10.2 Section Quiz. • 3. What is the volume of 0.35 mol of oxygen gas at STP? • 32 L • 64 L • 7.8 L • 16 L

  24. END OF SHOW

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