The gas molecules interact with one another
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.
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
Krypton is not an ideal gas because it deviates from the ideal gas law at high pressures and low temperatures due to its intermolecular interactions. At standard conditions, krypton behaves closely to an ideal gas, but as conditions vary, its non-ideal characteristics become more pronounced.
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.
High temperature; low pressure.
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
Make V explicit in the general for of the gas law: P.V = n.R.T then you get V = (n.R.T) / P
At absolute zero temperature, the volume of an ideal gas would theoretically be zero.
The gas molecules interact with one another
Make V explicit in the general for of the gas law: P.V = n.R.T then you get V = (n.R.T) / P
An ideal gas conforming to the ideal gas law (PV = nRT) would behave at all conditions of temperature and pressure. However, in reality, no gas perfectly conforms to the gas laws under all conditions.
There are ideal gases..