All Flashcards
What's the key difference between Isothermal and Adiabatic processes?
Isothermal: Constant temperature, heat transfer allowed (ΔT=0). | Adiabatic: No heat transfer, temperature can change (Q=0).
Define Internal Energy (U).
The total energy stored within a system, including the kinetic and potential energies of its particles.
Define First Law of Thermodynamics.
The change in internal energy (ΔU) of a closed system equals the heat added (Q) plus the work done on the system (W): ΔU = Q + W.
Define Isovolumetric process.
A thermodynamic process where the volume remains constant (ΔV = 0).
Define Isothermal process.
A thermodynamic process where the temperature remains constant (ΔT = 0).
Define Adiabatic process.
A thermodynamic process where no heat is transferred into or out of the system (Q = 0).
Define Isobaric process.
A thermodynamic process where the pressure remains constant (ΔP = 0).
Define Internal Energy (U).
The total energy stored within a system, including the kinetic energy of particles and the potential energy due to interactions between them.
What is an Isovolumetric process?
A thermodynamic process where the volume remains constant (ΔV = 0).
What is an Isothermal process?
A thermodynamic process where the temperature remains constant (ΔT = 0).
What is an Isobaric process?
A thermodynamic process where the pressure remains constant (ΔP = 0).
What is an Adiabatic process?
A thermodynamic process where there is no heat transfer (Q = 0) between the system and its surroundings.
Define the First Law of Thermodynamics.
The change in internal energy (ΔU) of a closed system equals the heat added (Q) to the system plus the work done (W) on the system: ΔU = Q + W.