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In an ideal gas compared to a real gas at very high pressure occupies?
A 'real' gas would occupy a higher volume as compared to the same amount of gas would have when 'idealistically' calculated by the 'ideal' gas law. The 'eigen' volume (its own molecular dimension) is to be taken in account at high pressure.
How do the particles in a real gas deviate from ideal gas behavior?
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.
Do real gases follow the ideal gas equation?
The gas which obeyed the gas laws at all conditions of temperature and pressure would be called an ideal gas. They don't actually exist. Real gases obey the gas laws approximately under moderate conditions. Some other points of distinction that can be considered are:Ideal gases are incompressible, non-viscous & non-turbulent.Real gases are compressible, viscous & turbulent.
How can one determine the volume of a gas using the formula for calculating gas volume?
To determine the volume of a gas using the formula for calculating gas volume, you would need to know the amount of gas in moles (n) and the gas constant (R), and the temperature (T) and pressure (P) of the gas. The formula for calculating gas volume is V (nRT) / P, where V is the volume of the gas. By plugging in the values for n, R, T, and P into the formula, you can calculate the volume of the gas.
Does a gas have a deifinite volume?
The volume of a gas is dependent on the pressure and temperature of the gas.
Can the volume of the particles in a real gas can be ignored?
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.
What At low temperatures and pressure how does the volume of a real gas compare with the volume of an ideal gas under the same conditions?
It is less
Would it be possible to cool a real gas down to zero volume?
No, it is not possible to cool a real gas down to zero volume due to the effects of quantum mechanics. As a gas is compressed and its volume decreases, the pressure and temperature would increase. Eventually, at a certain point known as the absolute zero of temperature, the gas would turn into a liquid or solid, rather than occupying zero volume.
In an ideal gas compared to a real gas at very high pressure occupies?
A 'real' gas would occupy a higher volume as compared to the same amount of gas would have when 'idealistically' calculated by the 'ideal' gas law. The 'eigen' volume (its own molecular dimension) is to be taken in account at high pressure.
A real gas differs from an ideal gas because the molecules of real gas have?
higher molecular volumes and exhibit intermolecular forces, such as van der Waals forces, that cause deviations from ideal gas behavior. These intermolecular forces affect the compressibility, volume, and pressure of a real gas, making it different from the assumptions of an ideal gas.
Can the volume of gas be zero if yes than how?
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.
What are two characteristics of an ideal gas that are not true of a real gas?
they have no volume and their molecular force of attraction is negligible
How do the particles in a real gas deviate from ideal gas behavior?
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.
How does an ideal gas diff from a real gas?
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).
What is the volume of the gas before and after cooled?
The volume of a gas - at constant pressure - is proportional to the absolute temperature, that is, to the temperature expressed in Kelvin. This relationship is only approximate for real gases, but it is close enough for most practical purposes.
Explain what is the difference between real gas molecules and ideal gas molecules by kinetic theory?
Real gas molecules have volume and experience intermolecular forces, while ideal gas molecules are treated as point particles with negligible volume and no intermolecular forces. In real gases, molecules have varying speeds and collision effects due to their volume and interactions, while ideal gases follow the assumptions of the kinetic theory perfectly due to their simplified behavior.
What is neglegible volume?
the negligible volume of a gas means that gas has a volume which is too little
