One mole of H2O(s) at −20∘C is subjected to a series of steps in an insulated system:
(a) Calculate the total energy, in kilojoules, required to complete steps 1–4 (the purely physical changes). Show each contribution separately before giving the sum.
(b) Determine the ratio of the energy required for the chemical decomposition in step 5 to the total energy calculated for the physical changes in part (a).
(c) Interpret the numerical ratio from part (b) in terms of the relative strengths of chemical bonds versus intermolecular forces in water.
(d) If the available energy supply were limited to 300kJ, identify which steps in the sequence could be completed and which could not. Justify your answer quantitatively.