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Kinetic Theory of Gases

Kinetic Theory of Gases. Gas is composed of molecules like little spheres placed far apart. Increase in temperature, increase in molecules’ speed which causes more collisions to happen. Increase in collisions, increase in pressure. Boyle’s Law

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Kinetic Theory of Gases

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  1. Kinetic Theory of Gases Gas is composed of molecules like little spheres placed far apart. Increase in temperature, increase in molecules’ speed which causes more collisions to happen. Increase in collisions, increase in pressure.

  2. Boyle’s Law “The volume of an enclosed dry gas varies inversely with its pressure, provided the temperature remains constant.” All pressures values must be in absolute. OR

  3. If the temperature of a gas is kept constant and pressure is doubled, the volume is reduced by half, the volume is reduced by half and the density doubles. Pressure and density are a direct relation OR

  4. Charles’ Law Gases expand and contract in direct proportion to the change in absolute temperatures, when the pressure is held constant. OR

  5. A balloon has a volume of 54.7 cu ft at a temperature of 756 deg K. What will happen when temperature drops to 500 deg K?

  6. If volume is constant, pressure and temperature are in direct proportion. OR

  7. Temperature and pressure must be in an absolute scale. A cylinder at 50 deg F has a pressure of 2000 psig. What will be the pressure when the cylinder heats to 100 deg F? Step 1: Convert to Rankine. Step 3: Plug into equation. Step 2: Convert to absolute pressure.

  8. General Gas Law Combine Boyle’s Law and Charles’ Law OR

  9. If the gas is not excessively different from those normally experienced on the earth’s surface, then the following equation holds true. Equation of state: Where R = constant for air = 53.345

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