[lapingarou]

   Hi everyone,

   This is my first message here so i'll try to be as clear as possible (or as my english allows me to be clear )). I have a question about the combustion of an hydrocarbon. The combustion of 1 mole of air leads to:

    R*B*CxHy + (0.21*O2+0.79*H2O) => a*CO2 + b*H2O + c*N2

with B the stoechiometric fuel/air ratio ; R the equivalence rationb ; and {a,b,c} the number of mole of products.


I would like to take into account the presence of nitrogen-oxyde (NOx). The new equation will be:

   R*B*CxHy + (0.21*O2+0.79*H2O) => a'*CO2 + b'*H2O + c'*N2 + d'*Nox


with a new atom balance for {a',b',c',d'}.


The fact is that i have an experimental value of the nox emission and air mass flow rate. It is something like:      Nox = 210ppm     and Qm_air = 0.03kg/s.

   question: what is the link between {d'} and those measure? I think about two solution:

      - d' = 210.e(-9)
      - d'=Qm_air/M_air*210.e(-9)    (with M_air the molar mass of fuel)


Is my problem finaly clear )? Hope that someone could help me.

   thank you
   Linda

[Borek]

0.21*O2+0.79*H2O

And not 0.79 N₂?

[lapingarou]

Hi borek,

  thank you for your answer. indeed it is   0.21.O2+0.79.N2