Chemical energetics: compare question

Three enthalpy changes for copper(II) sulfate are:

$$\ce{CuSO4(s) + aq -> CuSO4(aq)} \qquad \Delta H = -64.0\ \mathrm{kJ\,mol^{-1}}$$ $$\ce{CuSO4.5H2O(s) + aq -> CuSO4(aq)} \qquad \Delta H = +12.5\ \mathrm{kJ\,mol^{-1}}$$ $$\ce{CuSO4(s) + 5H2O(l) -> CuSO4.5H2O(s)} \qquad \Delta H = -76.5\ \mathrm{kJ\,mol^{-1}}$$

Compare the energy cycle linking these three changes. Without doing a calculation, describe the two routes from $\ce{CuSO4(s)}$ to $\ce{CuSO4(aq)}$, state how the three enthalpy changes are related, and explain what the signs of the hydration step and of the dissolution of the hydrated salt show about the relative stability of the anhydrous and hydrated forms.