BTueSep02 - Thermodynamics Kinetic Theory of Gases but...

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1 Thermodynamics Chemical Energy into Thermal Energy Kinetic Theory of Gases but first, a video
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2 The Kinetic Theory of Gases We assume the following: The gas consists of tiny particles Particles are points and have no volume There are no attractive or repulsive forces The particles are in continuous random motion Collisions result in a change in direction and velocity Collisions with the wall exert a force which causes pressure The collisions are perfectly elastic The average kinetic energy of the particles is proportional to the absolute temperature.
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3 A Particle in a Box l y x z
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4 The Particle (a bit of gas) The particle has mass m The velocity of the particle is u and it is a vector quantity, that is it has magnitude and direction. The particle has a velocity that can be resolved in all three dimensions x , y and z. To start with we will consider just one direction, the x direction. The impact of the particle on the wall gives rise to the pressure. (That was one of our assumptions).
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5 Can we calculate the pressure on one wall? YES! Pressure is force divided by area Force is the rate of change of momentum (Newton’s second law of motion) Momentum is mass times velocity.
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6 Momentum Momentum is a vector quantity, it has magnitude and direction. In a closed system it is conserved.
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