gas Heat conductionstate of matter

If a temperature difference is maintained across a fluid, a flow of energy through the fluid will result. The energy flow is proportional to the temperature difference according to Fourier’s law, where the constant of proportionality (aside from the geometric factors of the apparatus) is called the heat conductivity or thermal conductivity of the fluid, λ. Mechanisms other than conduction can transport energy, in particular convection and radiation; here it is assumed that these can be eliminated or adjusted for. The SI units for λ are J/m · s · K or watt per metre degree (W/m · K), but sometimes calories are used for the energy term instead of joules (one calorie = 4.184 J). At 20° C the thermal conductivity of water is 0.60 W/m · K, and that of many organic liquids is roughly only one-third as large. The thermal conductivity of air at 20° C is only about 2.5 × 10^-2 W/m · K. To a rough approximation, liquids conduct heat about 10 times better than do gases.

The properties of the thermal conductivity of dilute gases parallel those of viscosity in some respects. The most striking is the lack of dependence on pressure or density. Based on this fact, there seems to be no advantage to pumping out the inner chambers of thermos bottles. As far as conduction is concerned, it does not provide any benefits until practically all the air has been removed and free-molecule conduction is occurring. Convection, however, does depend on density, so some degree of insulation is provided by pumping out only some of the air.

The thermal conductivity of a dilute gas increases with increasing temperature, much like its viscosity. In this case, such behaviour does not seem particularly odd, probably because most people do not have a preconceived idea of how thermal conductivity should behave, unlike the situation with viscosity.

There are some differences in the behaviour of thermal conductivity and viscosity; one of the most notable has to do with mixtures. At first glance the thermal conductivity of a gaseous mixture seems to be as expected, since it falls between the conductivities of its components, but a closer look reveals an odd regularity. The conductivity of the mixture is always less than an average based on the number of moles (or molecules) of each component in the mixture. This appears to be related to the different effect that molecular weight has on thermal conductivity and viscosity. Light gases are usually better conductors than are heavy gases, whereas heavy gases are often (but not always) more viscous than are light gases. There also seems to be some correlation between molar heat capacity and thermal conductivity. The foregoing properties of thermal conductivity pose more puzzles that the kinetic theory of gases must address.