When considering air pressure level, do molecules' collision play a more important role on effecting air pressure than molecules' density? On the other words, whenever air pressure gets higher, it can be explained by
1) more molecules' collision occur at this moment, instead of
2) molecules' density gets higher

Which statement (1) or (2) is correct during higher air pressure?

Do you have any suggestions?
Thanks, to everyone very much for any suggestions (^v^)

I'm conflicted by your question


Molecular collision depends on the number of molecules per units3. If you have a high volume of molecules in 1 unit3, more collisions will occur.

What do you mean by molecule's density? Like an individual molecule?

1) there is 1000 molecule within 10 unit3
2) there is 1000 molecule within 1 unit3

In term of air pressure, case 2 would gets higher density within smaller volume, would case 2 gets higher air pressure under this situation?

Do you have any suggestions?
Thanks, to everyone very much for any suggestions (^v^)

Thanks for elaborating.

From the example you provided, if you keep the temperature constant, air pressure increases with density, because the more molecules per unit volume, the greater the push exerted by collisions.

Going back to the question you asked, which has a greater effect, number of collisions per unit time or the density of the molecules, for this you need the formula:

p = R r T

p is pressure,
r is density
T is temperature (in degrees Kelvin),
R is the specific gas constant, which varies from gas to gas.
For dry air, R is 287 J K-1 kg-1.

Try changing the variables to see which has a greater effect.

This very important relationship is known as the Equation of State, and simply means:

(1) for constant density, pressure increases with temperature (that is, if the molecules have a higher average kinetic energy, they exert a greater push on their surroundings);
(2) for constant temperature, pressure increases with density (the more molecules per unit volume, the greater the push exerted by collisions);
(3) for constant pressure, temperature and density are inversely related (that is, if there are fewer molecules in a given volume, they need to be travelling at a greater average speed to exert the same pressure).

Therefore, we can see that any change in any one variable is likely to cause changes in the others. For example, if we heat a mass of air, we increase its pressure, if the air is allowed to expand to equalise the pressure difference with the surrounding air, the density will decrease. When this happens, it will be lighter than the same volume of surrounding air, and will rise.

Refer to this link and I hope this clears it up

https://www.st-andrews.ac.uk/~dib2/climate/pressure.html

Thanks, to everyone very much for suggestions (^v^)

Hope you came to a conclusion!

You're welcome