How Does Heat Expansion Affect Gas Temperature?

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The discussion centers on the behavior of a monatomic ideal gas when heat is supplied, causing its volume to double and pressure to halve. It highlights the application of the ideal gas law, specifically the relationship between pressure, volume, and temperature. The final temperature of the gas can be determined using the equation (P1V1)/(T1)=(P2V2)T2, with R and n remaining constant. A key point is that the gas does not expand solely due to heat supply; instead, it absorbs heat from its surroundings during expansion. Understanding these principles is crucial for solving the problem accurately.
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Heat is supplised to a sample of a monatomic ideal gas at 40C. It is observed that the gas expands until its volume is doubled and the pressure drops to half of its original value. What is the final temperature of the gas? How do you solve? pv=nRt R and n are constant so do you have (P1V1)/(T1)=(P2V2)T2?
 
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KingTutATL said:
Heat is supplised to a sample of a monatomic ideal gas at 40C. It is observed that the gas expands until its volume is doubled and the pressure drops to half of its original value. What is the final temperature of the gas? How do you solve? pv=nRt R and n are constant so do you have (P1V1)/(T1)=(P2V2)T2?
You've got it. The question is a bit confusing because the gas does not expand due to the supply of heat. It draws heat from its surroundings as it expands.

AM
 

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