Under what conditions do real gases behave like ideal gases(obey the ideal gas laws)?
2007-10-19 01:23:45 · 5 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
gases at high temperatures and low densities are most likely to exhibit the properties of an ideal gas.
2007-10-19 01:29:05 · answer #1 · answered by Brian K² 6 · 2⤊ 0⤋
Just to add a bit...the ideal gas law assumes that ideal gases have no molecular volume and that all collisions between molecules are completely elastic. That is, that there is no intermolecular attraction between the molecules of the gas when they collide. Conditions of low pressure and high temperature minimize the non-ideal aspects of real gases.
2007-10-19 08:44:14 · answer #2 · answered by hcbiochem 7 · 0⤊ 0⤋
the gases which obey gas laws such as chales law ,boyles law,n gas equation are called ideal gases..
At high temperature low pressure gases behave as ideal gases
2007-10-19 08:36:48 · answer #3 · answered by chilly 1 · 1⤊ 0⤋
at high temperatures and low pressures - the high temperature means that the gas molecules will have enough energy to overcome any attractive forces that exist between the gas molecules - at low pressure, the gas molecules will be far apart and the volume of one molecule will be small compared to the volume of all the molecules
2007-10-19 08:33:25 · answer #4 · answered by chem geek 4 · 2⤊ 0⤋
at standard temperatur pressure conditions (STP)...under low pressures (i.e. near atmospheric) and temperatures (room temp) it also assumes that they are molecular non-reactive species
2007-10-19 08:29:01 · answer #5 · answered by Brent 3 · 0⤊ 0⤋