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The Mole – Volume Relationship

The Mole – Volume Relationship. Avogadro’s Hypothesis. equal volumes of gases at the same temperature and pressure contain the equal number of particles. Number of moles to volume(L) and volume(L) to moles.

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The Mole – Volume Relationship

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  1. The Mole – Volume Relationship

  2. Avogadro’s Hypothesis • equal volumes of gases at the same temperature and pressure contain the equal number of particles.

  3. Number of moles to volume(L) and volume(L) to moles • at standard temperature (0°C) and pressure (1 atmosphere), one mole of any gas has a volume of 22.4 L • this is called the molar volume of a gas

  4. Find the volume (in liters) of .60 moles of SO2 gas. .60 mol SO2 x 22.4 L SO2 1 1 mol SO2 = 13.0 L SO2 • Find the number of moles in 0.200 L of H2 gas. • 0.200 L H2 x 1 mole H2__ • 1 22.4 L H2 = 8.93 x 10-3 mol H2

  5. Volume to number of particles… and so on • Find the number of particles in 3.5 L of chlorine gas (Cl2). • 3.5 L Cl2x 1 mole Cl2_ x _6.02 X 1023 particles Cl2 • 1 22.4 L Cl21 mole = 9.41 X 1022 molecules Cl2 • Find the volume of 51.2 g of chlorine gas (Cl2). • 51.2 g Cl2x 1 mole Cl2_ x _22.4 L Cl2 • 1 71.0 g Cl2 1 mole = 16.2 L Cl2

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