Page 117 - Modeling of Chemical Kinetics and Reactor Design

Thermodynamics of Chemical Reactions 87

+
.
.
∆C =−62 54 4 635 ×10 −2 T −0 721 ×10 −5 T 2 J
.
p
mol K
723
∆H ( 723 K)= ∆H ( 298 K)+ ∫ ∆C dT
rxn
rxn
p
298
Substituting ∆H ( 298 K) and the parameters ∆a, ∆b, and ∆c in
o
rxn
Equation 2-110 gives
∆H ( 723 K) = ∆H ( 298 K)
rxn
rxn
723
+ ( − 2 − 5 T dT )
×
2
62 54 4 635 10
∫ − . + . × T 0 721 10
− .
298
∆a T T ) + (
2
2
∆H T ( )= ∆H o T ( )+ ( − ∆b T − )
T
rxnT rxnT R R R
2
∆c
3
3
+ ( T − )
T
R
3
(
∆H ( K)=− 62 54 723 298)
−
{
,
rxn 723 164 987+ − .
4 635 10 ( 723 − 298 )
−
×
2
2
2
.
+
2
.
0 721 ×10 −5 (723 3 − 298 3 )
− }
3
= –164,987 – 26,579.5 + 10,056.21 – 844.70
= –182,354.99
J
,
=−182 355
g mol CO
2