the molecules of a gas are constantly in a state of motion and the number of collision remains constant
the number of molecule of gas increases with increasing pressure
as the temperature increases, the number of collision made by the gas molecule remains constant
the molecules of gas are all identical and are very small in size
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Discussions (11)
D is correct for an ideal gas but incorrect for a real gas .. in the question no mention of an ideal gas ... therefore A is perfectly suited to be the answer to this question
The correct answer is:
D. the molecules of gas are all identical and are very small in size
Explanation:
According to the Kinetic Theory of Gases, some key assumptions include:
Gas molecules are very small compared to the distance between them.
Molecules are identical (for a given gas).
They are in constant random motion.
Collisions are elastic, but the number of collisions is not constant—it depends on conditions like temperature and pressure.
Why others are incorrect:
A: Molecules are in motion (true), but the number of collisions is not constant.
B: Number of molecules does not increase with pressure (unless gas is added).
C: Increasing temperature actually increases collisions, not keeps them constant.
So, D matches a valid assumption.
no, its not A because collision is not constant, it increases with increase in temperature
