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

the temperature of the gas must have increased

Step-by-step explanation:

As we know that

`v = \sqrt{(3RT)/(M)}`

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

`v = \sqrt{(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