No, that's why you call it real gas. For an ideal gas the size of the particle, that means the volume of interaction is zero, for real gases not. An effect of real gases is the cool down (or heat up) of an gas which is expanded (compressed). Another effect is that you can get liquids.
The ideal gas law does not specify the intermolecular forces between gas particles or the volume of the gas particles themselves. It also does not account for the presence of real gas behavior, such as deviations at high pressures or low temperatures. Additionally, the ideal gas law assumes that gas particles have zero volume and that they do not interact with each other.
According to the ideal gas law, the volume of individual gas particles is assumed to be zero. Of course, this isn't possible; all matter has volume. However, if we assume they have zero volume (along with collisions which are 100% elastic and statistically random motion) it makes the math a lot easier.
The state with the least number of particles in a certain volume would be a gas, as the particles in a gas are more spread out and have more kinetic energy compared to particles in liquids or solids. This results in fewer particles occupying a specific volume in a gas compared to a liquid or solid.
Ideal gases are gases with negligible intermolecular forces and molecular volumes. Real gases have intermolecular forces and have definite volumes at room temperature and pressure (RTP).
If the container is rigid, then its volume cannot change. However, if more gas particles are pushing on the walls, then it is the pressure that is changing.
Yes, a real gas has volume because its particles occupy physical space. Unlike an ideal gas, which is assumed to have no volume and incompressible point particles, real gases have finite molecular sizes and experience intermolecular interactions that result in volume occupancy.
The particles in a real gas deviate from ideal gas behavior due to interactions between the particles. In an ideal gas, the particles are assumed to have no volume and no interactions with each other. In a real gas, the particles have volume and can interact through forces such as van der Waals forces. These interactions can cause the gas to deviate from ideal behavior, especially at high pressures and low temperatures.
No, the volume of gas cannot be zero according to the kinetic theory of gases. Gas particles are in constant motion and have a non-zero volume because they occupy space. Even at extremely low pressures or temperatures, there will still be some volume occupied by gas particles.
The ideal gas law does not specify the intermolecular forces between gas particles or the volume of the gas particles themselves. It also does not account for the presence of real gas behavior, such as deviations at high pressures or low temperatures. Additionally, the ideal gas law assumes that gas particles have zero volume and that they do not interact with each other.
You can increase the volume of a gas by increasing the pressure applied to it. By compressing the gas into a smaller space, the gas particles will occupy a larger volume due to the increased pressure. This does not change the number or type of particles present in the gas.
Yes, particles in a gas can be compressed into a smaller volume by reducing the space between them. This will increase the pressure of the gas as the particles are forced closer together.
The volume of gas depends on the temperature, pressure, and number of gas particles present. These factors affect the amount of space the gas particles occupy.
According to the ideal gas law, the volume of individual gas particles is assumed to be zero. Of course, this isn't possible; all matter has volume. However, if we assume they have zero volume (along with collisions which are 100% elastic and statistically random motion) it makes the math a lot easier.
The state with the least number of particles in a certain volume would be a gas, as the particles in a gas are more spread out and have more kinetic energy compared to particles in liquids or solids. This results in fewer particles occupying a specific volume in a gas compared to a liquid or solid.
When the number of gas particles at constant pressure increases, the volume of the gas will increase due to the additional collisions between the gas particles and the walls of the container. This causes the gas to take up more space to accommodate the increased number of particles.
the gas
The particles are free