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6.6 The Volume of a Mole of a Gas

6.6 The Volume of a Mole of a Gas. One-mole amounts of different solid and liquid substances have different volumes. Example: Figure 6-7 – a mole of table sugar has a larger volume of a mole of water. The volume of a gas changes with temperature and pressure .

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6.6 The Volume of a Mole of a Gas

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  1. 6.6 The Volume of a Mole of a Gas • One-mole amounts of different solid and liquid substances have different volumes. • Example: Figure 6-7 – a mole of table sugar has a larger volume of a mole of water. • The volume of a gas changes with temperature and pressure. • Because of this, the volumes of gases are usually measures at standard temperature and pressure (STP)

  2. 6.6 The Volume of a Mole of a Gas • Standard Temperature and Pressure (STP) • Standard temperature is 0°C • Standard pressureis 101.3 kPa or 1 atm • At STP, 1 mol of any gas occupies a volume of 22.4 L. • This quantity is referred to as the molar volume of a gas and is measured at STP. • 22.4 L of any gas at STP is 1 mole of that gas, so it contains 6.02 x 1023 representative particles of that gas

  3. 6.6 The Volume of a Mole of a Gas • Would 22.4 L of one gas have the same mass as 22.4 L of another gas at STP? Why or why not? Hint: Image the two gases were hydrogen (H2) and oxygen (O2).

  4. 6.6 Example 8 – Moles to Volume • Determine the volume, in liters, of 0.600 mol sulfur dioxide, SO2, gas at STP. Unknown: Volume (L of SO2) Known: 0.600 mol SO2 1 mol SO2 = 22.4 L of SO2 at STP Solution: 0.600 mol SO2 1 22.4 L SO2 1.00 mol SO2 x = 13.4 L SO2

  5. 6.6 Example 9 – Volume to Moles • Determine the number of moles in 33.6 L of He gas at STP. Unknown: mol He Known: 33.6 L of He 1.00 mol He = 22.4 L of He Solution: 33.6 L He 1 1.00 mol He 22.4 L He x = 1.50 mol He

  6. 6.7 Gas Density and the gmm • The density of a gas is usually measured in the units g/L. • The experimentally determined density of a gas at STP is used to calculate the gram formula mass of that gas • density = mass/volume • density = molar mass/molar volume • For gases at STP, density = molar mass/22.4 L

  7. 6.7 Example 10 • The density of a gaseous compound of carbon and oxygen is 1.964 g/L at STP. Determine its gram formula mass. Is the compound CO2 or CO? Unknown: gfm (g) Known: 1.964 g/L; 1.964 g = 1 L Solution: 22.4 L 1 1.964 g 1 L x = 44.0 g

  8. 6.7 Example 10 • Is the compound CO2 or CO? gfm CO: 12 g/mol (C) + 16 g/mol (O) = 28 g/mol gfm CO2: 12 g/mol (C) + 2(16 g/mol) (O) = 44 g/mol Answer: The gas is CO2

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