The gas molecules interact with one another
The gas molecules interact with one another
An ideal gas has particles with zero volume that have no attractive or repulsive forces between them. Real gases have particles with a definite shape and volume. They also have weak attractive forces to each other. The larger the volume and the stronger the forces, the less ideal the gas will be.
1 mole of an ideal gas at STP occupies 22.4 liters. If STP is 'close' to the boiling point a real gas may deviate from ideal behavior and thus the volume will not be as predicted.
Make V explicit in the general for of the gas law: P.V = n.R.T then you get V = (n.R.T) / P
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.
V=nRT/P
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.
The gas molecules interact with one another
The gas molecules interact with one another
The volume is 22,710 980(38) litres for the ideal gas.
1 mole of an ideal gas at STP occupies 22.4 liters. If STP is 'close' to the boiling point a real gas may deviate from ideal behavior and thus the volume will not be as predicted.
1 mole of an ideal gas at STP occupies 22.4 liters. If STP is 'close' to the boiling point a real gas may deviate from ideal behavior and thus the volume will not be as predicted.
High temperature; low pressure.
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.
Make V explicit in the general for of the gas law: P.V = n.R.T then you get V = (n.R.T) / P
Make V explicit in the general for of the gas law: P.V = n.R.T then you get V = (n.R.T) / P
The gas molecules interact with one another
An ideal gas is assumed to have "point mass" - i.e. each molecule of gas occupies no intrinsic volume, thus the ideal gas is infinitely compressible since the molecules will never overlap as they are compressed like they would in a real gas.
Make V explicit in the general for of the gas law: P.V = n.R.T then you get V = (n.R.T) / P