RE: HEAT1=HEAT2 ?

["Rauber, Joel Phys" <RAUBERJ@mg.sdstate.edu>]

Hi Gang,
I'm back from my summer hiatus and once again find it to irresistable not to 
comment.
Ludwik wrote:
............................................................................
> Yes, the word heat has two conflicting meanings in many introductory 
physics
> textbooks. In thermodynamics it refers to that part of a thermal energy 
change
> which is due to a difference of temperatures, dT, between the inside and
> outside of a system. It is a path-dependent quantity, usually expressed in
> joules. In elementary physics on the other hand, heat is the name given to
> the quantity Q when the formula Q=c*m*dT is used to perform simple
> calorimetric calculations.  . . . .
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....

In a standard calorimetry experiment is the quantity of heat transferred, 
calculated from c*m*dt equal to the internal change that arises from a 
transfer of energy due to the difference of temperatures dT???  I.e. I see 
no contradiction in the two cases posed above, the reason is of course that 
in a standard calorimetry there is no dW term, (at least to good 
approximation and in so far as we are dealing with an ideal situation, blah 
blah blah, i.e. ignoring any work done in mixing the material in the 
calorimeter.)

Joel