Thermodynamics Trio:
A: Internal Energy (U): In thermodynamics, internal energy (also called the thermal energy) is defined as the energy associated with microscopic forms of energy. It is an extensive quantity, it is dependent on the size of the system, or on the amount of substance it contains.
B: Heat (Q): It the form of energy that is transferred between two substances at different temperatures. The direction of energy flow is from the substance of higher temperature to the substance of lower temperature.
C: Work Done (W): Work in thermodynamics is a measure of energy transfer that occurs when an object is moved by an external force. It is considered as energy in transit—energy cannot be stored or conserved, it can only be transferred.
Traditional Understanding: The first law of thermodynamics is all about energy conservation. It basically states that energy cannot be created or destroyed, only transferred or transformed. If a system has an increase in internal energy this increase is either due to work done on the system or due to heat put into the system.
Simplified Triadic Interpretations:
1. **Coexistence Triad and First Law of Thermodynamics**: The Coexistence Triad ( U ↔ Q ) ∧ ( Q ↔ W ) ∧ ( U ↔ W ) could be related to the first law of thermodynamics—the principle of conservation of energy. It states that energy can neither be created nor destroyed; it can only be transferred or changing from one form to another.
2. **Cycle Triad and Energy Transfer**: The Cycle Triad ( U → Q ) ∧ ( Q → W ) ∧ ( W → U ) captures the cyclic nature of energy transfer in a closed system. The internal energy (U) may change due to transfer of heat (Q) to or from the system or due to work (W) done by or on the system.
3. **Contingency Triad and Thermo Systems**: The Contingency Triad ( U → Q ) ∧ ( Q → W ) ∧ ( ¬U → ¬W ) can be associated with a system where work done by or on a system involves a corresponding increase or decrease in internal energy and heat.