Introduction To Thermodynamics First Law And Internal Energy
Key concepts for the “Introduction to Thermodynamics - First Law and Internal Energy”:
Zeroth Law of Thermodynamics
- Two systems in thermal equilibrium with a third system are in thermal equilibrium with each other.
First Law of Thermodynamics
- Energy cannot be created or destroyed, but can only be transferred or transformed from one form to another.
- For a thermodynamic system, the change in internal energy is equal to the heat added to the system minus the work done by the system.
Internal Energy
- The internal energy of a system is the sum of all the kinetic and potential energies of the particles within the system.
- Internal energy is dependent on the state of the system, and not on the path taken to reach that state.
Heat
- Heat is the transfer of thermal energy between two systems at different temperatures.
- Heat always flows from a higher-temperature system to a lower-temperature system.
Work
- Work is the transfer of energy between two systems through the application of force over a distance.
- Work can be done on a system by the surroundings, or by the system on the surroundings.
Isolated, Closed, and Open Systems
- An isolated system is one that does not exchange matter or energy with its surroundings.
- A closed system can exchange energy but not matter with its surroundings.
- An open system can exchange both energy and matter with its surroundings.
