The definition of the word Kinetic molecular theory is the collection of several rules that describe the behavior of gases.
A. The kinetic molecular theory relates the properties of a state of matter to the motion of its molecules.
The higher the kinetic energy of the molecules, the faster its movement will be. The state of a matter will depend on how fast the molecules move. When the molecules barely move, it will be packed tightly and its state will be solid. If the molecules kinetic energy rises, eventually they start moving around and the state will be liquid. If the kinetic energy rises further, the molecule will expand and changed into gas form.
1.The particles move faster, and their average kinetic energy increases.
If the temperature of gases are increase, the gas particles will gain more kinetic energy and they will begin to move randomly and haphazardly in the container that contains them. Temperature is directly proportional to increase in kinetic energy of gases.
2. The entire container because gases will expand to fill it.
Gases fills up containers and they assume the volume and shape of wherever they are put into. Therefore, the volume of occupied by a gas is actually the volume of the container they occupy. Gases are able to do this because they are free.
3. Because the attractive forces between gas particles are negligible, gas particles can glide easily past one another.
Gases acts fluid because they have little to no intermolecular attraction between them. Therefore they have low density and close to zero packing. This makes them easily glide past one another and this is why they act fluid.
Solids are arranged in a particular pattern. The molecules are close together and they vibrate about a fixed position. Ordered arrangements of particles of solid gives them their unique shapes.
5. Gas particles spread out to fill a container, leading to a low density of the gas.
Density is defined as the amount of substance i.e mass per unit volume. If you have more mass occupying a particular volume, then density will be high. For gases, they move to fill the containers that houses them and so they have low density.
6. Solids have low compressibility compared to liquids.
Gases are the most compressible form of matter. Solids are not easily compressible because their particles have a well ordered arrangement. Solids are rigid and do not readily move. Therefore, they readily restrain compressive forces on them. Liquids molecules moves about within the liquid. They are slightly compressible.
Option 3 is correct.
3. The molecular collisions are perfectly elastic.Explanation:
According to the kinetic molecular theory, the molecular collisions are perfectly elastic, so the the molecules of a gas striking with the wall of container are elastic and they are exerting considerable pressure on the walls of container. This pressure is actually exerted against the walls is less for real gases as compared to ideal gases.
The average kinetic energy of gas molecules increases with increasing temperature
There are gas molecules that move faster than the average
The average speed of gas molecules decreases with decreasing temperature
All the gas molecules in a sample cannot have the same kinetic energy
The average kinetic energy of the particles in an ideal monoatomic gas is given by:
k is the Boltzmann constant
T is the absolute temperature of the gas
While the rms speed of the particles in a gas is given by
R is the gas constant
T is the absolute temperature
M is the molar mass
Let's now analyze each statement:
- The average kinetic energy of gas molecules increases with increasing temperature --> TRUE. If we look at eq.(1), we see that the average kinetic energy is directly proportional to the temperature.
- There are gas molecules that move faster than the average --> TRUE. The distribution of the speed of the particles in a gas is spread around the rms speed, but of course not all the particles are moving at that speed: some particles are moving faster, while some are moving slower.
- The temperature of a gas sample is independent of the average kinetic energy --> FALSE. As we see from eq.(1), the two quantities are related to each other.
- The average speed of gas molecules decreases with decreasing temperature --> TRUE. As we see from eq.(2), the average speed is proportional to the square root of the temperature: so, when the temperature decreases, the average speed decreases as well.
- All the gas molecules in a sample cannot have the same kinetic energy --> TRUE. In fact, each particle will have a different kinetic energy, depending on its speed (different speed means also different kinetic energy).
The correct answer is 3. The molecular collisions are perfectly elastic.
Explanation- The rapidly moving particle of gas collides with the walls of the container. All these collision are perfectly elastic. The pressure exerted by the gas is due to this continuous collision and the force experienced per unit area of the walls of the container determines the pressure exerted by the gas.