Respuesta :
Answer: e. As the pressure increases, there are more collisions of helium atoms with the container wall.
Explanation:
We are given the information that helium gas is pumped into a rigid container at a constant temperature.
Due to this reason, there was a rise in the pressure of helium in the container. We should note that as the pressure rises, there are more collisions of helium atoms with the container wall.
The increase in the pressure of He atoms results in the increased collision of atoms with the wall. Thus, option E is correct.
The helium in the container is assumed to be an ideal gas. The ideal gas reaction is given as:
[tex]PV=nRT[/tex]
Where,
- P= Pressure
- V=volume
- n=moles
- R=Rydberg constant
- T=temperature
What happens to gas with an increase in pressure?
The ideal gas equation depicts that the gas is contained in a closed container. Thus, the moles, n of gas are constant. The pressure is pumped at a constant temperature, thereby T is also constant.
The R is a constant in the ideal gas equation. The increase in the pressure of the container results in the increased kinetic energy of the helium atoms.
The increase in the collisions is observed for the molecules with the container wall.
Thus, with the increase in pressure, the collisions in the atoms increase. Hence, option E is correct.
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