Basic Monatomic Ideal Gas Speed/Temperature Relationship

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Doubling the speed of every atom in a monatomic ideal gas results in a quadrupling of the temperature. This is due to the direct proportionality between temperature and kinetic energy. Since kinetic energy is proportional to the square of the speed, increasing the speed by a factor of two increases the kinetic energy by a factor of four. Therefore, the temperature in Kelvin would also increase by a factor of four. This relationship highlights the fundamental principles of thermodynamics in ideal gases.
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What would happen to the temperature (in Kelvin) if the speed of every atom in a monatomic ideal gas were doubled (specifically, what multiplication factor would be used)?
 
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Temperature is proportional to the kinetic energy. If the speed of every atom doubles, the temperature would rise by a factor of 4.
 
Thanks, that makes sense.
 

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