1. REAL VS IDEAL GASES

2. Ideal Gases Ideal gas may be defined as a gas which obeys the gas equation (PV=nRT) under all conditions of temperature and pressure; and hence the gas equation is also known as Ideal Gas Equation.

3. Real Gases However,no gas is perfect and the concept of perfect gas is only theoretical.Gases tend to show ideal behaviour more and more as the temperature rises above the boiling points of their liquified forms and the pressure is lowered.Such gases are known as real gases.Thus a real gas may be defined as a gas which obeys the gas laws under low pressure or high temperature.

4. Ideal GasReal Gas It obeys gas laws (PV=nRT) under all conditions of temperature and pressure. It obeys gas laws (PV=nRT) only at high temperature and low pressures. It is hypothetical i.e.does not exist. Nitrogen,helium and hydrogen which do not liquefy easily come nearest to behaving as ideal gases. All gases are real. Volume occupied by molecules is negligible as compared to volume of container The volume occupied by the molecules is not negligible as compared to the total volume of gas There is no intermolecular force of attraction between the molecules. The force of attraction are not negligible

5. Real gases obey the van der Waals equation where p is the pressure of the fluidpressure V is the total volume of the container containing the fluid a is a measure of the attraction between the particles b is the volume excluded by a mole of particles n is the number of moles R is the universal gas constant, gas constant T is the absolute temperatureabsolute temperature Correction for molecular attration Correction for volume of molecules

6. The van der Waals constants a and b are different for different gasses They generally increase with an increase in mass of the molecule and with an increase in the complexity of the gas molecule (i.e. volume and number of atoms) Substancea (L 2 atm/mol 2 )b(L/mol) He0.03410.0237 H2H2 0.2440.0266 O2O2 1.360.0318 H2OH2O5.460.035 CH 4 20.40.1383

7. Deviations From Ideal Gas Behaviour Plotting PV/RT for various gasses as a function of pressure, P: The deviation from ideal behavior is large at high pressure. The deviation varies from gas to gas. At lower pressures (<10 atm) the deviation from ideal behavior is typically small, and the ideal gas law can be used to predict behavior with little error.

8. Deviation from ideal behavior is also a function of temperature: As temperature increases the deviation from ideal behavior decreases. As temperature decreases the deviation increases, with a maximum deviation near the temperature at which the gas becomes a liquid.

9. Liquefaction of Gases For some gases boiling points and type of intermolec ular forces are given. GasesBoiling Point ( 0 C) Type of Intermolecular Forces H2OH2O100Hydrogen Bonding, Dipole- Dipole, London Forces CH 3 OH64.96Hydrogen Bonding, Dipole- Dipole, London Forces SO 2 -10Dipole-Dipole, London Forces Cl 2 -34.6London Forces CO 2 -78.5London Forces O2O2 -182.9London Forces F2F2 -188.1London Forces He-268.6London Forces

10. As the intermolecular forces are weaker, the gas is closest to ideal behaviour. As the strength of intermolecular forces increases, the gas liquefies and deviates from ideal behaviour.

11. JOULE THOMSON EFFECT Joule-Thomson effect, the change in temperature that accompanies expansion of a gas without production of work or transfer of heat. At ordinary temperatures and pressures, all real gases except hydrogen and helium cool upon such expansion; this phenomenon often is utilized in liquefying gases.

12. The phenomenon was investigated in 1852 by the British physicists James Prescott Joule and William Thomson (Lord Kelvin). The cooling occurs because work must be done to overcome the long-range attraction between the gas molecules as they move farther apart. Hydrogen and helium will cool upon expansion only if their initial temperatures are very low because the long-range forces in these gases are unusually weak.James Prescott JouleLord Kelvin

14. PHASE DIAGRAMS The simplest phase diagrams are pressure- temperature diagrams of a single simple substance, such as water. The axes correspond to the pressure and temperature. The phase diagram shows, in pressure- temperature space, the lines of equilibrium or phase boundaries between the three phases of solid, liquid, and gas.water axespressure temperature solidliquidgas

15. Critical Temperature Gases can be converted to liquids by compressing the gas at a suitable temperature. Gases become more difficult to liquefy as the temperature increases because the kinetic energies of the particles that make up the gas also increase. The critical temperature of a substance is the temperature at and above which vapor of the substance cannot be liquefied, no matter how much pressure is applied.

16. Vapor vs Gas A vapor condenses very readily to the liquid state under small changes of temperature or pressure or both, and constantly does so under ordinary conditions in nature. It may be said to be very close to the liquid state.

17. A gas, on the other hand, exists under ordinary conditions in the gaseous state. To change it to the liquid state extreme changes in gaseous and liquid state is required. A gas may be said to be far removed from the liquid state, and can not change to it under ordinary natural conditions.

18. Vapors are gases which can be liquefied, so a gas above its critical temperature can not be referred to as a vapor.

19. Helium: Critical temperature: -268 0 C. All our nature and life conditions exist above its critical temperature. We will consider it as a gas not a vapor.

20. Propane : Critical temperature: 97 0 C. This substance when in gaseous state will be considered as vapor.At room temperature it will remain gaseous. By placing it in a container and pressurizing it, we can turn it into liquid at room temperature.

21. Water: Critical temperature: 374 0 C. This substance when in gaseous state will be considered as vapor.At room temperature certain amount of water will be liquid. We can turn water into gas by placing it in a container and lowering the pressure.

22. Properties of Refrigerants It has a low boiling point, so that at room conditions it stays gaseous. It has high critical point so that it can be liquefied and vaporized under applicable pressure. It should be unreactive, cheap, consume less energy It should not be toxic, flammable, not cause environmental damage and corrosion

23. Helium: not a refrigerant. It has a low boliling and critical point Water: not a refrigerant. Liquid at room conditions. NH 3 :not a good refrigerant. It has a low boiling point and high critical point but it is toxic. CCl 2 F 2: not a good refrigerant. It has a low boiling point and high critical point but it damages ozon layer. Puron (50% difluorometan, 50%penta fluoro etan): a good refrigerant. It has a low boiling point and high critical point.