I would like to hear your opinion of the difference between heat and temperature. I teach in my class that the relation between temperature and heat is similar to that of voltage and current in electrical engineering. Or concentration and mass (Mass transfer), ... Some say that the temperature is a measure of heat. Others say that the heat Q divided by temperature T is the entropy. Probably all these answers are not fault. How is your opinion? Other interpretations?
From my understanding (I am still a student with much to learn):
Temperature is measure of the thermal energy of a system. Although the temperature of a body apparently has no upper limit, it does have a lower limit, i.e. 0 K When we say that a body is of a certain temperature, it does not imply that every molecule of that system has energy corresponding to that temperature, as the temporal state of the molecules is changing constantly by motion, thereby changing each molecule's energy content. If one averages the thermal energies of all the molecules in the system, we obtain what is commonly known as temperature, which is a measure of thermal energy. Internal energy, on the other hand, is frequently referred to as heat and more specifically, the heat content of the bodies.
Heat is the energy form that can be transferred from one system to another, observable by a change in temperature. Put simply, one is cause and other is its effect, akin to how a potential difference or voltage difference drives an electric current (as in your example), how pressure difference drives fluid flow or how a temperature difference/temperature gradient drives heat flow.
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