Question

The temperature of an ideal gas is directly proportional to the average kinetic energy of its molecules. If a container of an 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.

Answer 1

Answer:

the temperature of the gas must have increased

Explanation:

As we know that

$v = \sqrt{\frac{3RT}{M}}$

from this at room temperature the speed of air molecules is given as

$v = \sqrt{\frac{3(8.31)(300)}{0.029}}$

$v = 508 m/s$

now if the speed of the container was initially at

v = 2000 m/s

now we know that this speed is more than the speed of air molecules at room temperature

so here the temperature of the gas must have increased