Practice question

**Isobaric and isothermal** are fundamental thermodynamic processes, isobaric P constant horizontal line on P-V diagram, isothermal hyperbolic P = n R T/V, work equals area under curve, isothermal work larger than adiabatic for same volume change because pressure higher. Heat ( Δ Q ) is energy in transit due to a temperature difference, not a property of the system, while internal energy ( U ) is a state variable representing the total energy of the system's molecules. Heat is a process quantity; internal energy is a stored quantity. Using first law ΔU = Q - W, W = ∫ P dV, isobaric W = P