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What is the effect of adding heat to a closed system?
The internal energy of the system increases (ΔU increases), assuming no work is done by the system.
What is the effect of compressing a gas adiabatically?
The temperature of the gas increases because work is done on the system, increasing its internal energy, and no heat is allowed to escape.
What happens to the internal energy of an ideal gas during an isothermal expansion?
The internal energy remains constant because the temperature is constant, and for an ideal gas, internal energy depends only on temperature.
What is the effect of an isovolumetric process on work done?
Since there is no change in volume (ΔV = 0), no work is done (W = 0).
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).