“Chemical Thermodynamics: Numerical Practice” is available to Standard subscribers.
The calculations JEE asks most: work in reversible and irreversible expansions, Born-Haber and Hess cycles, bond enthalpies, and ΔG from ΔH and ΔS, with a full timed paper.
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Work in reversible and irreversible changes: The same expansion can do very different amounts of work. Against a constant pressure, w = -p_ext ΔV. More stages give more work, and the reversible path gives the most. In compression the reversible path needs the least. An adiabatic change has q = 0, so ΔU = w, and ΔH = ΔU + Δn_g RT links the two for reactions.
Enthalpy cycles in practice: Hess's law lets you find any enthalpy you cannot measure from ones you can. From combustion enthalpies you get enthalpies of formation. Comparing measured values with bond enthalpies gives the resonance energy of benzene. A Born-Haber cycle gives the lattice enthalpy of a salt, and neutralisation shows what it costs to ionise a weak acid.
Spontaneity by numbers: At a phase change, ΔS = ΔH/T. The surroundings gain entropy ΔS_surr = -ΔH/T, and a change is spontaneous when the total rises. A reaction with ΔH and ΔS of the same sign turns around at T = ΔH/ΔS. ΔG° = -RT ln K gives the equilibrium constant, and ΔG = ΔG° + RT ln Q tells which way any mixture moves.