3268 kJ are required to change 1 mole of ethanol into its gaseous atoms.

C₂H₅OH(g) → 2C(g) + 6H(g) + O(g)

a. Calculate the entropy change of the surroundings during this process when it is carried out at 150°C.

b. Explain why the total entropy change of this reaction is likely to be negative.

c. When ethanol undergoes combustion, carbon dioxide and water are formed.

C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l)            ΔH^θreaction = –1367 kJ mol^–1

Calculate the total standard entropy change for this reaction. (Values for S^θin J K^–1 mol^–1: C₂H₅OH(l) = 160.7, CO₂ =213.6, H₂O(l) = 69.90, O₂(g) = 205.0)