I Why Do Volume-Temperature Curves of Ideal Gases Intersect at Absolute Zero?

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All volume-temperature curves of an ideal gas intersect at the same point on the temperature axis due to the relationship between temperature and average kinetic energy. As the size of gas particles approaches zero in a model, the behavior aligns with that of an ideal gas. This model supports Charles's Law, which states that volume is directly proportional to temperature. The zero point on the temperature scale corresponds to zero average kinetic energy of the gas particles. While these models are approximations, they effectively describe gas behavior under many conditions.
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Why do all the volume temperature curves of an ideal gas intersect at the same point on the temperature axis ?
 
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If you decide to model a gas as a large collection of tiny balls in a large otherwise empty space then, as you reduce the ball size toward zero you get the behavior of an ideal gas.

If you decide to model temperature as the average kinetic energy per ball in such an arrangement then you get the Charles law. The zero point on the temperature scale is the point where the average kinetic energy per ball is zero.

Neither model is exactly correct for real gasses. But they are good approximations for many purposes.
 
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