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Kinetic Molecular Theory of Gases Gases consist of molecules that are constantly moving through space in strait lines, randomly, and with various speeds
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Kinetic Molecular Theory of Gases The average kinetic energy of the gas molecule is proportional to the absolute (K) temperature Meaning: the higher the temperature, the faster the gas particles move
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Kinetic Molecular Theory of Gases The gas molecules collide with each other without loosing any kinetic energy – like billiard balls
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Kinetic Molecular Theory of Gases The molecules volume is tiny compared to that of the container – the assumption that in comparison the gas molecules take up not volume is used
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Kinetic Molecular Theory of Gases Gas molecules have no attraction between themselves
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Kinetic Molecular Theory of Gases The collisions against the sides of the container constitute the pressure of the gas
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Pressure Pressure = force / area SI unit = pascal (Pa) = 1 newton / m2 Atmospheric pressure – column of air pressing down on a given point
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BarometerManometer
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STP = Standard Temperature and Pressure STP 1atm = 760 mm Hg = 760 torr = 101,325 Pa
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