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Some of my heretical ideas about heat were presented last year at a Gordon
Conference on the teaching of thermodynamics. I shall send you the relevant
sections as an attachment. Anyone who wants the full text can write to me,
but it is not for the faint of heart.
Consider the following piece of nonsense, taken from a famous textbook of
physical chemistry. Hydrogen and oxygen are enclosed in a rigid, insulated
container. They react to form water. The book says that in this process
heat is absorbed? Where on earth from? From the ether? By anyone's
definition, this is an adiabatic process, one in which no "heat is
absorbed or emitted (ugh!)". In fact, on a previous page of this textbook
an adiabatic process is so defined. But then the author forgets what he
said previously and presents us with an adiabatic process in which is
"heat is absorbed" but who knows from where.
Since heating and working appear symmetrically in first law, why is it
that we don't refer to the amount of work in a body or the work added to
it or absorbed by it or the work content? We don't, because we recognize
that working is a process, and work is not a substance, but heat still
survives as a substance, a thing.
Consider the following simple demonstration. I rub my hands together
vigorously, thereby experiencing the feeling of warmth. There are two ways
of describing this: heat was generated (despite this being an essentially
adiabatic process ); or, the temperature of my hands increased.
How do I measure the amount of heat generated?
By letting it drip into a can?
So let's get rid of heat as a substance once and for all from thermodynamics
and teach our students that heating is a process in which a system's
energy increases or decreases by virtue of a temperature difference
between it and its surroundings.