C2H4(g)+X2(g)?C2H4X2(g) where X2 can be Cl2, Br2, or I2. Use the thermodynamic d

Question

C2H4(g)+X2(g)?C2H4X2(g) where X2 can be Cl2, Br2, or I2.
Use the thermodynamic data given below to calculate ?H? for the halogenation reaction by Cl2 at 35?C.
Compound ?H?f(kJ/mol) ?S?f(J/mol?K)
C2H4Cl2(g) -129.7 308.0
C2H4Br2(g) -38.3 330.6
C2H4I2(g) 66.5 347.8
?H=
?S=
?G=
Kp= C2H4(g)+X2(g)?C2H4X2(g) where X2 can be Cl2, Br2, or I2.
Use the thermodynamic data given below to calculate ?H? for the halogenation reaction by Cl2 at 35?C.
Compound ?H?f(kJ/mol) ?S?f(J/mol?K)
C2H4Cl2(g) -129.7 308.0
C2H4Br2(g) -38.3 330.6
C2H4I2(g) 66.5 347.8
?H=
?S=
?G=
Kp=

Explanation / Answer

dH = dHf products - dHf reactants

dH = dHf C2H4X2 - dHf X2 - dHf C2H4

dH = -129.7 -0 - 52.3

dH = -182 kJ/mol

dS = dS products - dS reactants

dS = dSf C2H4X2 - dSf X2 - dSf C2H4

dS = 308 - 223 -219.5

dS = -134.5 J/mol/K

dG = dH -TdS

dG = -182 x 1000 + 308 x 134.5

dG = -140. 974 kJ/mol

dG is -140.574 kJ/mol

dG = -RT lnk

-140 .974 x 1000 =-8.314 x 308 lnkp

kp = 6.94 x 1023

Kp is 6.94 x 1023

So Kp is 6.94 x 10^23

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