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lesson 4.4 heat

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Gas pressure, temperature and volume in terms of  gas molecules. The kinetic theory of gases was proposed to explain the gas laws. The basic assumptions are:  1. All gases are made up of a very large number of tiny molecules. 2. These molecules are constantly moving around randomly at high speeds. 3. The molecules collide elastically with anything they meet. If they hit the inner walls of the container , they bounce off again at the same speed. 4. The molecules are so small and so far apart that they almost never collide with each other. So the volume of the gas molecules themselves is negligible with the volume of container, that is, almost all the gas is empty space. 5. They do not exert any forces on each other , but move randomly. There is no intermolecular attractive forces. Intermolecular forces of repulsion act only during collisions between molecules; the duration of collisions is negligible compare compared with the time interval between collisions. How the gas pressure is produced?  Based on the assumptions of kinetic theory of gases , molecules of a gas will occupy the entire available space and collisions occur between molecules and the walls of container. Imagine a molecule of mass m approaching one wall with velocity , v . Its momentum = mv. It rebounds with velocity (-v) because it experiences an elastic collision. Its momentum now is - mv. So the change of momentum = 2mv According to Newton’s second law of motion , force is exerted on the wall of container because force is the rate change of momentum ( F = change of momentum  ) time As the result gas pressure is produced because  by the definition of pressure; Pressure is Force per unit area ( P = F )  A Hence the gas pressure  in the container is the total force , produced by the collision between molecules and the walls of container. 27 L ESSON  4- Understanding  

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