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Hello.
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Today we're going to talk about chapter 12, question 23, which asks us to relate charles's law, which is v1 over t1 equals v2 over t2 for an ideal gas, and we need to relate that to the kinetic molecular theory of a gas.
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So first, we'll just state what the kinetic molecular theory is.
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The kinetic molecular theory is the idea that gases have an average kinetic kinetic energy, that is related to the temperature of the gas, which causes the molecules to move and just kind of bounce around in their container randomly.
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So, for example, this gas has these molecules moving, bouncing off of each other, bouncing off the walls of the container, and so on.
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And this i've drawn here, it's just label, this is a piston that can be pushed back with enough force.
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And so this has, say, a pressure on the outside of, so p out is one atmosphere, and p inside at the moment is also one atmosphere.
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And so we're interested in what happens if we increase the temperature.
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And so if we increase the temperature, so we'll say that this is t1, we'll just say we increase temperature.
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Now we have more kinetic energy by the kinetic molecular theory.
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Our gases are more energetic.
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And so if we redraw our little setup, we've got our piston.
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Let's draw our gas first.
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We've got our gas molecules...