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Compare Isothermal and Adiabatic processes.
Isothermal: Constant temperature, heat transfer allowed. Adiabatic: No heat transfer, temperature can change.
Differentiate between work done *by* the system and work done *on* the system.
Work done BY the system: Volume increases (expansion), W is negative. Work done ON the system: Volume decreases (compression), W is positive.
How do you calculate work done by a system at constant pressure?
W = -PΔV, where P is pressure and ΔV is the change in volume.
Describe the steps to determine the change in internal energy of a system using the First Law of Thermodynamics.
1. Identify the heat added to the system (Q). 2. Determine the work done on the system (W). 3. Apply the formula ΔU = Q + W.
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.