Which of the following relations are correct? (A) ΔU = q + pΔV (B) ΔG = ΔH - TΔS (C) ΔS = q rev T (D) ΔH = ΔU - ΔnRT Choose the most appropriate answer from the options given below :

Step-by-step solution

The Gibbs free energy can be written as a function of enthalpy and entropy as follows, (B) G = H - TS At constant T ΔG = ΔH - TΔS (A) According to first law of thermodynamics, ΔU = Q + W If we apply constant P and reversible work. W = - P ∆ V ΔU = Q - PΔV (C) By definition of entropy change dS = dq rev T At constant T ΔS = q rev T Enthalpy can be written as a function of internal energy, pressure and volume as follows, (D) H = U + PV For ideal gas equation, PV = nRT H = U + nRT At constant T ΔH = ΔU + ΔnRT