613 Appendix G Kinetics Primer Consider a general reaction: or equivalently, (G.1) comprising r i moles of reactants R i and p k moles of products P k . Then we may write a law of mass action as (G.2) If the sign is negative, then the reaction consumes the species with time rather than produces them. We may also define the reaction rate for species k as rr k : (G.3) where is the molar volume [L 3 /N] and the reaction rate has units of [N/L 3 ]. For a constant volume (density) reaction, the equation reduces to (G.4) where the brackets indicate the molar concentration of the enclosed species. rr pp 11 22 11 22 RR PP++↔++$$ rp jj j m kk k n R == ∑∑ ↔ 11 P −=− = = 11 11 12 12 r dN dt r dN dt p dN dt p dN dt R1 R2 P1 P2 $$ rr r V dN dt p V dN dt k kk =− = 11 11 ˆˆ Rk Pk ˆ V rr r d dt p d dt k k k k k =− ⎡ ⎣ ⎤ ⎦ = ⎡ ⎣ ⎤ ⎦ 11 RP © 2006 by Taylor & Francis Group, LLC 614 Modeling of Combustion Systems: A Practical Approach Usually, one defines a reaction coordinate known as the conversion (x k ), having the property that for species k the reaction starts at x k = 0 and ends at x k = 1. The general definition is (G.5) where N k,0 is the starting number of moles of species k, and N k is the con- centration at some particular conversion of interest. Thus, N k,0 is a constant and N k is a variable. We may also write (G.6) For constant density, we have , where [k] is the concentration of species k, and [k 0 ] is the starting concentra- tion. We may write the conversion for any particular species and relate it to any other species according to (G.7) Or in terms of a single conversion (say, x R1 ), we may write (G.8) For constant density, we may write (G.9) (G.10) x NN N k kk k = − , , 0 0 NxN kkk =− () 1 0, x kk k k = ⎡ ⎣ ⎤ ⎦ − ⎡ ⎣ ⎤ ⎦ ⎡ ⎣ ⎤ ⎦ 0 0 kxk k ⎡ ⎣ ⎤ ⎦ =− () ⎡ ⎣ ⎤ ⎦ 1 0 N r x N r x N p R R R R P10 1 1 20 2 2 10 1 ,, , ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ = ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ ==$ ⎛⎛ ⎝ ⎜ ⎞ ⎠ ⎟ = ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ =x N p x P P P1 20 2 2 , $ x N N r r x N N r p x N R R R R P R P1 20 10 1 2 2 10 10 1 1 1 ==== , , , , $ PP R P 20 10 1 2 2 , , N r p x =$ RR P RR 10 1 1 20 2 2 ,, ⎡ ⎣ ⎤ ⎦ ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ = ⎡ ⎣ ⎤ ⎦ ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ == r x r x $ 110 1 1 20 2 2 ,, ⎡ ⎣ ⎤ ⎦ ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ = ⎡ ⎣ ⎤ ⎦ ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ = p x p x PP P $ x r r x RR R R P R 1 20 10 1 2 2 10 10 = ⎡ ⎣ ⎤ ⎦ ⎡ ⎣ ⎤ ⎦ == ⎡ ⎣ ⎤ ⎦ ⎡ , , , , $ ⎣⎣ ⎤ ⎦ = ⎡ ⎣ ⎤ ⎦ ⎡ ⎣ ⎤ ⎦ = r p x r p x 1 1 1 20 10 1 2 2PP P R , , $ © 2006 by Taylor & Francis Group, LLC Kinetics Primer 615 We may also substitute mole fractions for concentrations using (G.11) For combustion in furnaces, the ideal gas law applies: (G.12) where are the total moles of the reaction. This gives (G.13) We may also write as a function of conversion: (G.14) Typically, we use Equation G.8 or Equation G.10 to recast Equation G.14 in terms of a single conversion. ky P RT k ⎡ ⎣ ⎤ ⎦ = N V P RT k ∑ = ˆ N k ∑ ˆ V RT P N k = ∑ N k ∑ NxN kkk ∑∑ =− () 1 0, © 2006 by Taylor & Francis Group, LLC . by Taylor & Francis Group, LLC 614 Modeling of Combustion Systems: A Practical Approach Usually, one defines a reaction coordinate known as the conversion (x k ), having the property that for. 613 Appendix G Kinetics Primer Consider a general reaction: or equivalently, (G.1) comprising r i moles of reactants R i and p k moles of products P k . Then we may write a law of mass action. molar volume [L 3 /N] and the reaction rate has units of [N/L 3 ]. For a constant volume (density) reaction, the equation reduces to (G.4) where the brackets indicate the molar concentration of