Answer:
No
Explanation:
The equation of state for ideal gases tells that:
[tex]pV=nRT[/tex]
where
p is the gas pressure
V is the gas volume
n is the number of moles of the gas
R is the gas constant
T is the absolute temperature
In this problem, we have a fixed mass of gas. This means that the number of moles of the gas, [tex]n[/tex], does not change; also, the volume V remains the same, and R is a constant, this means that
[tex]p\propto T[/tex]
So, as the pressure increases, the temperature increases.
However, here we want to understand what happens to the average distance between the molecules.
We have said previously that the number of moles n does not change: and therefore, the total number of molecules in has does not change either.
If we consider one dimension only, we can say that the average distance between the molecules is
[tex]d=\frac{L}{N}[/tex]
where L is the length of the container and N the number of molecules. Since the volume of the container here does not change, L does not change, and since N is constant, this means that the average distance between the molecules remains the same.
