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There are two containers of equal volumes, each filled with a different gas. Both containers have the same number of moles of gas and are at the same temperature. The molecules of gas in container 1 are four times more massive than the molecules of gas in container 2. The number of moles in container 2 is increased until it is a factor of 4 larger than the number of moles in container
1. The volume and temperature of container 2 remain unchanged. After increasing the number of moles in container
2: Which container, 1 or 2, has a higher pressure, or are they the same? Which container, 1 or 2, has a higher average (rms) speed of gas molecules, or are they the same? Which container, 1 or 2, has a higher average kinetic energy of gas molecules, or are they the same? Which container, 1 or 2, has a higher thermal energy, or are they the same?

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Answer:

Molecules in container 2 has a higher pressure.

Molecules in container 2 has a greater rms speed.

Molecules in container 2 has a greater kinetic energy.

Molecules in container 2 has a greater thermal energy.

Explanation:

At constant volume and temperature, The number of moles of a gas is proportional to its pressure.

The lower the pressure, the lesser the rms speed of molecules, kinetic energy of the molecules and thermal energy of the molecules, hence the answer above.