Practice question

**Adiabatic process** no heat exchange Q=0, first law ΔU = -W, for ideal gas P V^γ = constant, T V^{γ-1}= constant, P^{1-γ} T^{γ}= constant, γ = C_p/C_v = (f+2)/f, monatomic γ=5/3, diatomic γ=7/5. Work done W = (P₁V₁ - P₂V₂)/(γ-1), temperature changes due to work. In an isobaric process ( P = constant ), heat added ( Δ Q ) increases internal energy ( Δ U ) and does work ( W = P Δ V ) due to volume expansion, as per the First Law: Δ Q = Δ U + P Δ V . Using first law ΔU = Q - W, W