How gas laws are violated by real gases?
Assumptions: First, ideal gases have molecules or atoms that take up no space. Second, the atoms or molecule of ideal gases neither attract nor repel one another. At high pressure or low temperature, volumes decrease, and atoms or molecules of real gases are so close together that they “try to occupy the same place at the same time.” Also, London forces tend to cause gas atoms or molecules to attract one another more than they would otherwise. Water molecules are polar, so dipole-dipole forces and hydrogen bonding cause them to attract one another more than they would.
