Consider the box below that contains a single atom of an ideal gas.
a. Assuming that this gas atom is moving, describe how it creates pressure inside the container.

b. Now consider the two containers below, each at the same temperature. If we were to measure the gas pressure in each container, how would they compare? Explain your answer.

c. Consider the two containers below, labeled C and D, one with an ideal gas atom and one with ideal gas molecules, each at the same temperature. The gas molecule has more mass than the gas atom. How do the pressures of the two containers compare? Why?

d. For the containers C and D above, which would have the higher root-mean-square (rms) molecular speed? How does the difference in rms speeds support or contradict the answer you obtained above when you compared the pressures?
e. Consider containers E and F below. How do the pressures in these containers compare? Be sure to explain your answer.

f. Consider containers G and H below, one with a gas atom and one with a gas molecule. As before, the gas molecule has more mass than the gas atom. Explain how the pressures in these containers compare.

g. Now think about the containers below, I and J. How do the pressures in these containers compare? Be sure to justify your answer.

h. Finally, how do the pressures in containers K and L compare?

Transcribed Image Text:

T 100 K T=200 K T= 100 K T=200 K T=200 K T= 100 K T= 200 K T 100 K