The reaction, C 2 H 6 (g) + Cl 2 (g) àC 2 H 5 Cl (g) + HCl (g), occurs in a cont
ID: 702806 • Letter: T
Question
The reaction, C2H6(g) + Cl2(g) àC2H5Cl (g) + HCl (g), occurs in a continuous flow reactor. 100 mol/hr of ethane and 125 mol/hr chlorine gas @ 25°C are fed to the reactor. Assume complete reaction of ethane. The reactor exit stream temperature is 200°C. Calculate the moles of each component of the feed and exit streams and the extent of reaction z. Calculate the heat released or absorbed (specify which) from the reactor using the heat of reaction method. The chloroethane heat capacity can be found in Perry's. For the Cpvalues from Table B.2 in your text, you may use just the “a” and “b” terms for simplicity.
Explanation / Answer
as given in the question feed has only two components ethane and chlorine
feed stream
100 moles/hr C2H6 and 125 moles/hr Cl2
in terms of mole fraction
C2H6 mole fraction 0.444
Cl2 mole fracton 0.556
for exit stream in terms of moles and mole fraction
C2H6 00 moles/hr and 00
Cl2 25 moles/hr and 0.111
C2H5Cl 100 moles/hr and 0.444
HCl 100 moles/hr and 0.444
extent of reaction for ecch of the species is same
z = 100
Cp(C2H6) = 52.98 KJ/(Kmol.K)
Cp(Cl2) = 29.2125 KJ/(Kmol.K)
Cp(C2H5Cl) = 62.78 KJ/(Kmol.K)
Cp(HCl) = 30.8 KJ/(Kmol.K)
heat of formation of Chloro ethane -105 KJ/mol
heat relesed when 100 mol of chloroethane formed 10500 KJ
heat consumed by 25 moles of chlorine to raise the temp from 25 to 200 = 25*29.2125*175 = 129.318 KJ
heat consumed by 100 moles of hydro-chloric acid to raise the temp from 25 to 200 = 100*30.8*175 = 539 KJ
heat consumed by 100 moles of chloroethane to raise the temp from 25 to 200 = 100*62.78*175 = 1098.65 KJ
total heat consumed = 1766.968 KJ
heat release during reaction = 10500 KJ
heat removed from the reactor = 10500 - 1766.968 = 8733.032 KJ
8733.032 KJ of heat is removed and release to the enviroment
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