Which of the following is true of gases?
A. Gases are not easily compressed because of expansion and limited space between particles.
B. Gases mix easily because of their high kinetic energy and low intermolecular forces.
C. Gas particles diffuse easily because of their low fluidity and high intermolecular forces.
D. Gas particles spread out to fill a container because of their high density and high kinetic energy.

B. Gases mix easily because of their high kinetic energy and low intermolecular forces

Explanation:

Gases have higher kinetic energy compared to solid and liquid because the large intermolecular spaces makes a large amount of movement between particles possible. The movements of the particles exhibits kinetic energy.

Gases are highly compressible because its particles aren’t tightly packed together. The intermolecular spaces are large and makes it easier for the gas particles to be compressed in a space which makes option A incorrect.

Gases have Low intermolecular molecules which explains why they aren’t tightly packed together which makes C incorrect.

Gases have a low density because the particles aren’t tightly packed together unlike the solids which are tightly packed together and denser than the liquid and gas which makes option D incorrect

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

i think the answer is terrae but not 100 percent sure. ▓▬▬ §