Chem homework due tomorrow:
Under what conditions would you predict that real gases least approximate ideal gas behavior? Explain why real gases behave least like ideal at the conditions stated.
2006-10-30 02:29:50 · 3 answers · asked by natrgrrl 2 in Science & Mathematics ➔ Chemistry
An ideal gas is a hypothetical gas consisting of identical particles of negligible volume, with no intermolecular forces. Also the atoms or molecules of the gas undergo perfectly elastic collisions with the walls of the container and each other.
Real gases do not exhibit these exact properties. The approximation breaks down at high pressures and low temperatures, where the intermolecular forces play a greater role in determining the properties of the gas.
2006-10-30 02:40:29 · answer #1 · answered by cordefr 7 · 2⤊ 1⤋
Real gases do not follow all postulates of the Kinetic Theory of gases
At low pressure and high temperature they behave most like ideal gases.
But at high pressure and low temperature they do not follow the following
1) There is no force of attraction or repulsion between the molecules of gas
2) The volume of the molecule itself cannot be neglected in comparison to the total voume of the gas
Hence real gases dont behave like ideal gases and dont follow the ideal gas equation
2006-10-30 03:13:00 · answer #2 · answered by Anonymous · 3⤊ 0⤋
Because the molecules of a real gas take up space (volume) and have an interaction between them (van der waals force). When the moleculesare closest together they act least like an ideal gas.. High pressure and low temperature would cause this.
2006-10-30 02:38:31 · answer #3 · answered by The Cheminator 5 · 4⤊ 1⤋