Illustrate (draw) the thermodynamic cycles for the acid dissociation of both HCl and HF. Classify each cycle as exergonic or endergonic. Do your calculated values agree with the observed strengths of each acid in water? Use the given experimental values below to answer this part of the question:

The aqueous solvation enthalpy of H+ is -1091 kJmol-1. The solvation energy of HX(g) ? HX(aq) is approx. -40 kJmol-1. The ionization energies of HCl(g) and HF(g) are 1393 kJmol-1 and 1553 kJmol-1 respectively.