Question

Liquid EO has ΔH°f =-77.4 kj/mol and ΔH° for its vaporization 5 569.4 J/g. (b) 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?

Answer 1

Final temperature if the average specific heat capacity of the products is 2.5 J/g·°C is 1302.57°C

Given reaction:

C₂H₄O(g) → CH₄(g) + CO(g)

Now,

 Given data for this reaction is :

ΔH°f =-77.4 kJ/mol

ΔH°vaporization =569.4 J/g

                           = 569.4J/g × 44.0g/mol

ΔH°vaporization= 25.082 kJ/mol

Now,

   ΔH°vaporization = H(vapor) -  H(liquid)

   25.082 = H(vapor) + 77.4 kJ/mol

  H(vapor) = -52.318 kJ/mol

Again,

  ΔH°rxn = ( H( CO(g))) + (H(CH₄(g))) - (H( C₂H₄O(g)))

               = -110.5 - 74.87 + 52.318

  ΔH°rxn = -133.053 kJ/mol

Now,

  Given

T₁= 93°C = 366K

We know that,

Q= mcΔT

133.053 × 10³ = 44 × 2.5 × (T₂ - 93)

 T₂ = 1302.57°C

Thus, from the above conclusion we can say that , Final temperature  if the average specific heat capacity of the products is 2.5 J/g·°C is 1302.57°C .

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

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