they have no volume and their molecular force of attraction is negligible
Not true. It applies to real gases that are exhibiting ideal behavior. Any gas that is not 'close' to its boiling and is at a 'low' pressure will behave like an ideal gas and Boyle's Law can be applied. Remember there is no such thing as an ideal gas, so when Boyle did his experiments and came up with his law he was using a real gas, probably just air.
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).
The molecules of real gas have some volume and some attraction for each other.
Real gases are those we encounter in the real world- hydrogen oxygen, nitrogen, argon, water vapour. An ideal gas is one that obeys the ideal gas law, usually expressed as PV=nRT. No real world gas follows this law although it is a good predictor of their behaviour as pressure, P, volume, V, temperature, T and number of moles, n, change.
Real gases approach ideal behavior at high temperature and low pressure. In this Condition gases occupy a large volume and molecules are far apart so volume of gas molecules are negligible and intermolecular force of attraction(responsible for non ideal behavior) become low. So gases approach ideal behavior.
No, no real gas is actually an ideal gas.
In an ideal gas molecules interact only elastically.
That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.
Not true. It applies to real gases that are exhibiting ideal behavior. Any gas that is not 'close' to its boiling and is at a 'low' pressure will behave like an ideal gas and Boyle's Law can be applied. Remember there is no such thing as an ideal gas, so when Boyle did his experiments and came up with his law he was using a real gas, probably just air.
The gas molecules interact with one another
If gas molecules were true geometric points (ie had zero volume) AND had zero intermolecular interaction (such as attraction or repulsion), then the gas would obey the ideal gas law. Gases composed of small, non-interactive molecules (such as helium gas) obey the ideal gas law pretty well (as long as the gas is low density and temperature is rather high). For non-ideal gases, at least two correction factors are often used to modify the ideal gas law (correcting for non-zero volume of gas molecule and intermolecular attraction) such as in the Van der Waals equation for a real gas.
An ideal gas is an abstraction - a simplification. No real gas behaves exactly like an "ideal gas". The reason an ideal gas is used is because (a) the math is simpler, and (b) this is close enough for real gases, in many cases. Thought this is often not stated explicitly, we can safely assume that an "ideal gas" is supposed to remain a gas, regardless of the temperature and pressure.
Ideal gas law states that there are no inter molecular attractions between gas molecules and that ideal gas does not occupy space therefore having no volume. However, a real gas does have intermolecular attractions and does have a volume.
In an ideal gas there is no attarcation between molecules. There is no such thing as an ideal gas it is a model that approximates the behaviour of real gases.
A real gas is a type of gas that is different than an ideal gas. They have completely different interactions between their molecules.
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).
The molecules of real gas have some volume and some attraction for each other.