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jobsism
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I've noticed that almost every good conductor of electricity, is also a good conductor of heat, except for certain exceptions like Graphite. Why is this so? I can't seem to associate electron flow with heat conduction.
Gordianus said:Check the Wiedemann-Franz law that explains how the ratio of thermal to electrical conductivity in metals is almost a constant
jobsism said:Ah, thank you for your reply! I understand the law, but I'm still confused on how electrical conduction contributes to thermal conduction. I'm thinking, that in good electricity conductors, there are more number of free electrons, the motion of which causes them to acquire higher thermal energy. But is this what allows higher heat conduction?
Both qualities are related to the ability of a material to transfer energy. In the case of a good conductor of electricity, it allows the flow of electrons easily, while in a good conductor of heat, it allows the transfer of thermal energy.
Yes, it is possible. For example, materials like copper and silver are excellent conductors of both electricity and heat, while materials like rubber and wood are good insulators of electricity but not of heat.
The atomic and molecular structure of a material plays a significant role. Materials with a highly ordered and dense structure tend to be good conductors of both electricity and heat, while those with a more disordered and loosely packed structure are usually poor conductors.
Yes, some materials like diamond and silicon carbide have a high thermal conductivity but a low electrical conductivity. This is due to the nature of their atomic bonds, which allow for efficient heat transfer but not for electron flow.
Good conductors of electricity are essential for the functioning of electronic devices, electrical wiring, and power transmission. Good conductors of heat are used in applications such as cooking, heating, and cooling systems. They are also crucial in industries that require precise temperature control, such as in metallurgy and chemical manufacturing.