Chemistry Final Exam- Kinetic Molecular
Theory
Latest Update 2023 a+
Use the kinetic-molecular theory to explain each of the following properties of
... [Show More] gases:
a. expansion
b. fluidity
c. low density
d. compressibility
e. diffusion - ANS-a. gas particles move rapidly in all directions without significant
attraction between them
b. the attractive forces between gas particles are insignificant so gas particles glide
easily past one another
c. particles are much farther apart in the gaseous state, providing less basis for a strong
density
d. during compression, initially far-apart particles are crowded closer together
e. the random and continuous motion of molecules carries them throughout the
available space
Describe the conditions under which a real gas is most likely to behave ideally - ANS-at
very high pressures and low temperatures; most likely to hold true for gases whose
particles have little attraction for each other (noble gases)
How does the kinetic-molecular theory explain the pressure exerted by gases? - ANSThe greater the number of molecules, the greater the number of collisions at a constant
temperature, which ultimately leads to the greater the pressure of the gas (and viceversa)
What happens to gas particles when a gas is heated? - ANS-the particles move faster
with increasing temperature and as a result, collide more
Describe the liquid state according to the kinetic-molecular theory - ANS-Liquids have
the medium energy level of the three states. They have enough energy for their
molecules to break free from their solid lattice but not enough to separate from being in
groups of molecules. They move around slowly and randomly in groups with a moderate
level of kinetic energy to power them
Properties of liquids - ANS-Relatively high density
Relative incompressibility
Ability to diffuse
Surface tension
Evaporation and Boiling
How does the kinetic-molecular theory explain the following properties of liquids:
Continues... [Show Less]