thermodynamics einstein assumption corrected nernst theorem

Breakthrough in Thermodynamics Corrects a Long-Standing Einstein Assumption

A Modern Take on Nernst's 1905 Entropy Observation

Professor José Martin-Olalla of the University of Seville has authored a paper in The European Physical Journal Plus, directly associating Nernst's 1905 observation on diminishing entropy exchange at low temperatures with the second law of thermodynamics—deepening our theoretical grasp of absolute zero behaviour in physical systems.

Resolving a 120-Year-Old Scientific Puzzle

The study resolves a long-standing issue dating back 120 years, while also extending the theoretical consequences of the second thermodynamic principle, which dictates the universe's rising entropy. Importantly, it challenges and corrects an assumption introduced by Albert Einstein more than a century ago, marking a notable refinement in classical thermodynamic thought.

Historical Background of Nernst's Theorem

Early 20th-Century Exploration of Absolute Zero

The challenge surrounding Nernst's theorem emerged in the early 20th century during investigations into the behaviour of matter near absolute zero (-273°C). For his pioneering work in this domain, Walther Nernst received the 1920 Nobel Prize in Chemistry.

Nernst's Argument for the Inaccessibility of Absolute Zero

Nernst explained that if absolute zero were reachable, it would enable the construction of an engine converting all heat into work, defying the entropy principle. Therefore, he concluded its inaccessibility and demonstrated his theorem in 1912.

Einstein's Response and Reinterpretation

Einstein promptly challenged the demonstration, insisting the engine it relied upon was impractical and irrelevant to the second law's validity. He thus reassigned the theorem to a third, distinct principle of the thermodynamics. That view, however, no longer holds under contemporary analysis.

Martín-Olalla's Modern Reformulation

Virtual Engines and Thermodynamic Consistency

In his analysis, Professor Martín-Olalla highlights two subtleties overlooked by Nernst and Einstein: while the second law of thermodynamics formally necessitates Nernst's hypothetical engine, it must remain a virtual construct—one that neither absorbs heat nor performs work and crucially, does not contravene the second principle.

Absolute Zero and Entropy Exchange

By combining both concepts, one may deduce that entropy exchange approaches zero as temperature nears absolute zero—consistent with Nernst's theorem—and that absolute zero itself remains fundamentally unattainable.

Revisiting the Concept of Temperature

Martin-Olalla points out that one of thermodynamics' fundamental challenges is to distinguish between the flet experience of temperature—the perceptions of hot and cold—and its theoretical, measurable definition. In the debate between Nernst and Einstein, temperature was simply an empirical parameter, with the condition of absolute zero defined by a gas's pressure or volume nearing zero.

Redefining Thermodynamic Proofs

Entropy's Unique Value at Absolute Zero

"In formal terms, the second law of thermodynamics offers a more precise conception of temperature's natural zero—unrelated to sensory perception, but instead tied to Nernst's hypothetical, purely virtual engine. This shift significantly alters how the theorem is to be proven."

Heat Capacity Cancellation and Entropy Clarification

According to the study, the cancellation of heat capacities near absolute zero—first outlined by Nernst in 1912—is the sole general property not evidently derived from the second law. Martin-Olalla contends that the second law already implies a unique entropy at absolute zero and that the vanishing heat capacities merely confirm this value to be zero.

Academic Reception and Future Outlook

The professor remarks that this publication marks an initial step towards wider acceptance of a new perspective. "My thermodynamics students were the first to encounter this demonstration. I hope the article increases its visibility, though I am aware that academic circles often change slowly."

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