# Problem: 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 = 569.4 J/g. External heating causes the vapor to decompose at 10 bar and 93°C in a distillation column. What is the final temperature if the average specific heat capacity of the products is 2.5 J/g•°C?

###### FREE Expert Solution

Recall: The enthalpy of vaporization ΔH˚vap is the amount of heat needed to completely vaporize 1 gram of a compound. It's given by:

The specific heat capacity C is the amount of heat needed to change the temperature by 1 ˚C of 1 gram of a compound. It's given by:

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###### Problem Details

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 = 569.4 J/g.

External heating causes the vapor to decompose at 10 bar and 93°C in a distillation column. What is the final temperature if the average specific heat capacity of the products is 2.5 J/g•°C?