Intermolecular_forces Gas

when gases compressed, intermolecular forces shown here start play more active role.

as discussed earlier, momentary attractions (or repulsions) between particles have effect on gas dynamics. in physical chemistry, name given these intermolecular forces van der waals force. these forces play key role in determining physical properties of gas such viscosity , flow rate (see physical characteristics section). ignoring these forces in conditions (see kinetic-molecular theory) allows real gas treated ideal gas. assumption allows use of ideal gas laws simplifies calculations.

proper use of these gas relationships requires kinetic-molecular theory (kmt). when gas particles possess magnetic charge or intermolecular force gradually influence 1 spacing between them reduced (the hydrogen bond model illustrates 1 example). in absence of charge, @ point when spacing between gas particles reduced can no longer avoid collisions between @ normal gas temperatures. case increased collisions among gas particles include fixed volume of gas, upon heating contain fast particles. means these ideal equations provide reasonable results except extremely high pressure (compressible) or high temperature (ionized) conditions. notice of these excepted conditions allow energy transfer take place within gas system. absence of these internal transfers referred ideal conditions in energy exchange occurs @ boundaries of system. real gases experience of these collisions , intermolecular forces. when these collisions statistically negligible (incompressible), results these ideal equations still meaningful. if gas particles compressed close proximity behave more liquid (see fluid dynamics).