Thermodynamics

No heat exchange with surroundings, Q = 0, PVᵞ = constant, ΔU = -W

In adiabatic process: (1) System is thermally isolated, so Q = 0, (2) Equation of state is PVᵞ = constant, (3) From first law: ΔU = Q - W = 0 - W = -W, (4) Temperature changes during adiabatic process.

ΔU = Q - W, Energy cannot be created or destroyed, Heat and work are equivalent forms of energy, Q = ΔU + W

First law states: ΔU = Q - W or Q = ΔU + W. It's a statement of energy conservation. Heat and work are interconvertible. However, complete conversion of heat to work is impossible (second law limitation).

200 J

Using first law: ΔU = Q - W. Given: Q = +500 J (heat absorbed), W = +300 J (work done by system). Therefore: ΔU = 500 - 300 = 200 J. Internal energy increases by 200 J.

Qc/W

Coefficient of Performance (CoP) = Qc/W, where Qc is heat extracted from cold reservoir and W is work input. It measures how much heat can be extracted per unit work input.