Thermodynamic related question

The temperature of an ideal gas is directly proportional to the average kinetic energy of its molecules. If a container of ideal gas is moving past you at 2000 m/s. is the temperature of the gas higher than if the container was at rest? Explain your reasoning. *Thermodynamics

Easy Math Editor

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Comments

The Temperature would be same if the container is moving or is at rest. This is because, the temperature of the gas depends only on the random motion of the gas molecules. Any systematic motion of the gas molecules (like kept in a container that moves with some velocity) doesn't affect the temperature. Hence the temperature is same.

Saurabh Dubey - 8 years, 1 month ago

When we are talking about an ideal gas what matters is the molecules' kinetic energy with respect to the center of its mass.That remains the same no matter if the system is moving(since both the molecules and the center of the mass are moving) or if it is at rest.So the temperature remains the same in both cases.

Avraam Aneleitos - 8 years, 1 month ago

the temp will change only when the velosity of random motion with respect to each other changes not with respect to ground..

Himank bhalla - 8 years, 1 month ago

Temperature of an ideal gas increases only when Microscopic energy(internal energy) increases . Bulk motion ( movement of centre of mass ) will result only in kinetic energy increase of the whole system

shashank srivastav - 6 years, 1 month ago

Math	Appears as
Remember to wrap math in `\(` ... `\)` or `\[` ... `\]` to ensure proper formatting.
`2 \times 3`	$2 \times 3$
`2^{34}`	$2^{34}$
`a_{i-1}`	$a_{i-1}$
`\frac{2}{3}`	$\frac{2}{3}$
`\sqrt{2}`	$\sqrt{2}$
`\sum_{i=1}^3`	$\sum_{i=1}^3$
`\sin \theta`	$\sin \theta$
`\boxed{123}`	$\boxed{123}$