mike.Albert99 said:Yes, exactly. The ideal gas molecule has no structure, so it can't rotate or vibrate. All it can do it move in three dimensions. f=3. Atomic gasses (at least the ones that don't make dimers) approximate this case and differ from the ideal primarily only in that they take up space reducing the available volume. More complicated molecules can vibrate and rotate and each independent motion is another degree of freedom where energy can be stored. The gas has more capacity to store energy as a function of temperature.
You can edit your posts.mike.Albert99 said:I just wanted to correct myself
mfb said:You can edit your posts.
The Kinetic Theory of Gases is a scientific model that explains the behavior of gases based on the motion of their individual molecules. It states that gas molecules are in constant, random motion and that the temperature of a gas is directly proportional to the average kinetic energy of its molecules.
According to the Kinetic Theory of Gases, gas molecules are in constant motion and collide with each other and the walls of their container. These collisions create pressure and cause the gas to expand and fill its container. Gas molecules also have different speeds and directions of motion, leading to their random motion.
The Kinetic Theory of Gases is based on the following assumptions: 1) Gas particles are considered to be point masses with no volume, 2) Gas molecules are in constant, random motion, 3) Collisions between gas molecules are perfectly elastic, meaning there is no loss of energy during collisions, and 4) Gas molecules do not exert attractive or repulsive forces on each other.
The Kinetic Theory of Gases states that as the temperature of a gas increases, the average kinetic energy of its molecules also increases. This means that the gas molecules will move faster and collide more frequently, resulting in an increase in pressure and volume.
The Kinetic Theory of Gases explains the relationship between pressure, volume, and temperature using the ideal gas law: PV = nRT. This equation states that the pressure and volume of a gas are inversely proportional to each other, while the pressure and temperature are directly proportional to each other. This relationship is known as Boyle's Law and Charles' Law, respectively, and can be explained by the behavior of gas molecules according to the Kinetic Theory.