Quantum Mechanics Cannot be Consistent with both of the First and Second Laws of Thermodynamics
Thomas Alexander Meyer
In quantum mechanics there are many transitions of particles which can be shown to conserve energy and momentum, but they fail to maintain consistency with the second law of thermodynamics, that heat must be lost to the environment in all heat transforms. To put it simply, because quantum mechanics is a theory of irreducible quanta which cannot be broken down into further divisible components, then the transition from one quanta to another is a transition which by definition cannot lose energy to an additional environment. For these transitions to obey the second law, it would require that there be an additional environment which gains heat energy in the transition, and such an environment could only be a "more fundamental" theory (which does not exist). Hence we abandon the second law of thermodynamics in preference of the first.
The laws of thermodynamics may roughly be stated as follows;
The first Law: dE = dQ + dW (also known as the law of conservation of energy) This law states that when we have a closed system where one body performs work upon another body, the total gain of internal energy of the body acted upon, dE, is equal to the total heat lost by the acting body (and thus gained by the body acted on), dQ, added to the total work performed on the body acted on, dW.
The Second Law: dS/dt = (1/T)dQ/dt > 0 (also known in many other forms) This law states that for a closed system with a transformation occurring with only irreversible processes, that the time rate of change of entropy, dS/dt, must be positive. The maximum state of entropy is thermodynamic equilibrium. This law may be restated for the case where only reversible processes take place, dS/dt = 0.
Is quantum mechanics nothing more than the presence of the equality?
July 22, 2013.