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Gases

Gases. Properties of Gases. Fluidity - Gas particles move around freely with negligible attraction to fill the shape of their container.

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Gases

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  1. Gases

  2. Properties of Gases • Fluidity - Gas particles move around freely with negligible attraction to fill the shape of their container. • Molar Volume - Gases are over 99% empty space. As a result, the size of the particles does not affect the volume. Equal amounts of any gas will occupy almost the exact same volume.

  3. Properties of Gases • Compressibility- Gases can easily change volume by placing a force on its container. (Solids and liquids cannot) • Diffusion - Mixing of 2 gases due to their random motion. All gases diffuse, but at different rates.

  4. Properties of Gases • Pressure – Gas particles are moving very fast and when they collide with their surroundings, they exert an outward force. Due to expansion, gases will flow until pressure is equalized. (ex: if a plane loses cabin pressure, the air will rush out until the pressure is equalized)

  5. Pressure Pressure is measured in: a. atmospheres (atm) b. millimeters of mercury (mm Hg) c. pascals (Pa) Atmospheric Pressure: 1.00 atm = 101.3kPa = 760 mm Hg

  6. Pressure If you increase the amount of gas in a container, you will increase the pressure of the gas. (ex: adding air to your tires increases the pressure)

  7. Pressure Dalton’s Law of partial pressures - The pressure of a mixture of gases is equal to the sum of their individual partial pressures. Ptotal = P1 + P2 + P3…. Pair = Pnitrogen + Poxygen + Pcarbon dioxide + Pwater vapor…

  8. Pressure Based on this table, if a chemical reaction done inside an enclosed container were to consume all of the oxygen, what would be the new pressure in kPa?

  9. Pressure A vacuum is created when all of the gases are removed from a volume. Because there are no particles, there is no air pressure. (Empty space has been created.) A partial vacuum is any volume with less pressure than the surrounding air, but not a complete vacuum.

  10. Pressure Total Vacuum = 0 atmospheres > 0 atm 1 atm > Partial Vacuum

  11. In many gas equations, you will be given conditions of “STP.” S STP = Standard Temperature and Pressure T P Standard Temperature = 0 C or 273 K Standard Pressure = 1.00 atm 101.3 kPa 760 mm Hg

  12. Pressure and Volume Boyle's Law – At constant temperature, the pressure of a gas is inversely proportional to its volume.

  13. Pressure and Volume Boyle's Law – At constant temperature, the pressure of a gas is inversely proportional to its volume. Inhaling – your lungs expand their volume creating low pressure. Air then rushes in to equalize the pressure. Exhaling – your diaphragm compresses your lungs into a smaller volume creating high pressure. Air then is expelled to equalize the pressure.

  14. Pressure and Volume Boyle's Law – At constant temperature, the pressure of a gas is inversely proportional to its volume. Graph P1 V1 = P2 V2

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