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Ethylene oxide (EO) is prepared by the vapor-phase oxidation of ethylene. Its main uses are in the preparation of the antifreeze ethylene glycol and in the production of poly(ethylene terephthalate), which is used to make beverage bottles and fibers. Pure EO vapor can decompose explosively:
Liquid EO has ΔH°f =-77.4 kj/mol and ΔH° for its vaporization 5 569.4 J/g. (a) Calculate ΔH°rxn for the gas-phase reaction.

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Ethylene oxide (EO) is prepared by the vapor-phase oxidation of ethylene. Its main uses are in the preparation of the antifreeze ethylene glycol and in the production of poly(ethylene terephthalate), which is used to make beverage bottles and fibers. Pure EO vapor can decompose explosively. ΔH°rxn for the gas-phase reaction is -133.0kJ/mol.

What is Ethylene Oxide?

  • Ethylene oxide is an organic compound with the formula C₂H₄O.
  • Ethylene oxide is a colorless and flammable gas with a faintly sweet odor.
  • ethylene oxide easily participates in a number of addition reactions that result in ring-opening.
  • Ethylene oxide is isomeric with acetaldehyde and with vinyl alcohol.

Uses of Ethylene Oxide:

  • Ethylene oxide is a surface disinfectant that is widely used in hospitals.
  • Adhesives
  • Agricultural insecticide
  • Antifreeze
  • Chemicals used to create fabrics for clothes, pillows and carpets
  • Cosmetics
  • Detergents
  • Fiberglass used in jet skis, bowling balls and other products
  • Herbicide
  • Household cleaners
  • Industrial cleaners
  • Medicines

Now,

  EO(l) → EO(g)

ΔH°vaporization = 569.4J/g(44.05g/mol)(1kJ/1J) = 25.08kJ/mol

Now,

ΔH°vaporization = { ΔH°f ( EO(g))} - {ΔH°f ( EO(l))}

25.08kJ/mol ={ ΔH°f ( EO(g))} - { (1mol)(-77.4kJ/mol)}

ΔH°fEO(g) = -52.32kJ/mol

Now,

EO(g) → CH₄(g) + CO(g)

ΔH°rxn =  [ΔH°f{CH₄(g)}] + [ΔH°f[CO(g)}] - [ ΔH°f{EO(g)}]

             = -74.87-110.5 +52.32

             ΔH°rxn= -133.0kJ/mol

Thus, from the above conclusion we can say that, ΔH°rxn for the gas-phase reaction is -133.0kJ/mol.

Learn more about Ethylene oxide here: https://brainly.com/question/14638014

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