Page 73 - Modeling of Chemical Kinetics and Reactor Design

Reaction Mechanisms and Rate Expressions 43

and

C + C = C (1-185)
O * N * T

Therefore,

C * = C − C * (1-186)
T
O N
Substituting Equation 1-186 into Equation 1-184 gives
T (
kC C − C ) = k C C
1 N 2 N * 2 N * O 2

kC N 2 C − k C N 2 C N * = k C N * C O 2
1
T
2
1
Therefore,
kC C T
1
C * = N 2
N kC N 2 + k C O 2 (1-187)
2
1
The net rate of formation of nitric oxide is:

+ ( r ) = k C C + k C C (1-188)
NO net 1 O * N 2 2 N * O 2
( )
= kC C −C + k C C
1 N 2 T N * 2 N * O 2

 kC C   kC C 




= kC  C T − 1 N 2 T  + kC  1 N 2 T 
2
1
 kC N 2 + k C O 2  O 2  kC N 2 + k C O 2 
N 2




2
2
1
1
 kC C T 
1
= kC C +( k C − k C ) N 2
1 T N 2 2 O 2 1 N 2 
 kC N 2 + k C O 2 
2
1
2kk C C O C N
12
= 2 2
T
kC N 2 + k C O 2 (1-189)
2
1