DIFFERENCE BETWEEN REAL GAS AND IDEAL GAS (IN POINTS)
|Ideal gas||Real gas|
|Molecules have negligible volume in comparison to the Total volume of the gas.||Volume of molecules is very small but not negligible in comparison to the total volume of the gas.|
|Collision between two molecule is elastic that is energy and momentum during the collision remain conserved||Collisions between molecules in real gas are not perfectly elastic.|
|There is no mutual force of attraction or repulsion between the molecules of ideal gas therefore ideal gas can't be liquefied.||There is force of attraction between the molecules of real gas therefore can be liquefied at high pressure and low temperature.|
|Ideal gas obeys PV = nRT (ideal gas equation )|
Real gas obeys vander walls equation.
|This gas follows all gas laws at all temperature and pressure conditions.||This gas does not follow gas laws at all temperature and pressure conditions. However, a real gas behaves ideally at high temperature and low pressure conditions.|
1 Ideal gas has no volume, and no forces of attraction between the molecules. it obeys PV =nRT,But a real gas has volume, and no forces of attraction between the molecules, and it does not obey PV=nRT
2 An ideal gas is infinitely compressible, a real gas will condense to a liquid at some pressure.
3 The particles of an ideal gas lose no energy to its container. A real gas conducts and radiates heat, thereby losing energy.