Etude de la combustion de gaz de synthèse issus d'un processus de ...
Etude de la combustion de gaz de synthèse issus d'un processus de ... Etude de la combustion de gaz de synthèse issus d'un processus de ...
Numerical simulation of a syngas-fuelled engine dV ⎛rc −1⎞ ⎛ ϕcosθ ⎞ = V TDC sinθ 1 dθ ⎜ 2 ⎟ + 2 2 ⎝ ⎠ ⎜ 1 − ϕ sin θ ⎟ ⎝ ⎠ (6.6) The mass fraction of each burned zone is defined as mbi , xbi , = ( i = 1,..., n) m (6.7) with the result for the total burned zone x b m = =∑ x (6.8) n b m i = 1 b, i tel-00623090, version 1 - 13 Sep 2011 The mass conservation equation is also applied to the cylinder charge, assuming zero blow-by, providing dm dm dm dm dm u b u bn , = + = + = 0 (6.9) dθ dθ dθ dθ dθ The previous relation has been derived assuming that the mass of each of the already burned zones remains constant after its combustion: dm b,i /dθ = 0 (i=1,…, n-1), resulting for the rate of change of mass of the total burned zone: n b θ = ∑ i 1 b, i θ = b, n θ (6.10) = dm d dm d dm d Also, the perfect gas state equation is applied to each zone. pV = m RT ( j = u, b − b ) (6.11) j j j j 1 n 6.1.2 Chemical composition and thermodynamic properties The unburned zone is considered to be a mixture of air and fuel, while also allowance is made for the presence of residual gas trapped in the engine cylinder. The composition and thermodynamic properties of the unburned mixture during compression and combustion are determined from the values of pressure, temperature, fuel–air equivalence ratio and residual gas mass fraction (Ferguson, 1986). After the start of combustion and until the end of expansion at EVO, the combustion products of each burned zone consist of a set of eleven chemical species: (1) CO 2 , (2) 170
Chapter 6 H 2 O, (3) N 2 , (4) O 2 , (5) CO, (6) H 2 , (7) H, (8) O, (9) OH, (10) NO, and (11) N, which are considered to be in chemical equilibrium. The calculation of their concentrations and, subsequently, each zone’s thermodynamic properties is based on the values of pressure, temperature and fuel–air equivalence ratio. For this reason, the atom balance equations of the C–H–O–N system are considered along with the following eight equilibrium reactions (Ferguson, 1986): H + O ⇔ H O 1 2 2 2 2 CO + O ⇔CO 1 2 2 2 CH + 2O ⇔ CO + 2H O 4 2 2 2 H + O ⇔OH 1 1 2 2 2 2 O + N ⇔ NO 1 1 2 2 2 2 (6.12) tel-00623090, version 1 - 13 Sep 2011 1 2 1 2 1 2 H O N 2 2 2 ⇔ H ⇔ O ⇔ N The various thermodynamic properties (specific enthalpy, specific internal energy, specific volume, specific heat capacity at constant pressure) and thermodynamic derivatives (derivative of logarithmic specific volume with respect to logarithmic temperature and pressure) of the unburned and burned mixtures, needed for the calculations, are computed according to the mole fraction of each species and the gas mixture rule. For this purpose, the well established coefficients (Heywood, 1988) of the polynomial curves that have been fitted to the various species thermodynamic data from JANAF tables are used. For the evaluation of specific internal energy of species i, the following relation can be applied according to JANAF Table thermodynamic data (Gordon and McBride, 1971; Heywood, 1988): 5 ⎡⎛ ain n ⎞ ⎤ ui( T) = Rsi ⎢⎜ ∑ T ⎟+ ai6 −T⎥ ⎣⎝ n= 1 n ⎠ ⎦ (6.13) where constants a in for the above polynomial relation can be found, for example, in (Ferguson, 1986; Heywood, 1988). Two sets of data are available for constants a in , one for temperatures up to 1000 K and another for temperatures from 1000 to 5000 K. The reference temperature is 298 K. Also, h( T) = u ( T) + R T (6.14) i i si 171
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Chapter 6<br />
H 2 O, (3) N 2 , (4) O 2 , (5) CO, (6) H 2 , (7) H, (8) O, (9) OH, (10) NO, and (11) N, which are<br />
consi<strong>de</strong>red to be in chemical equilibrium. The calcu<strong>la</strong>tion of their concentrations and,<br />
subsequently, each zone’s thermodynamic properties is based on the values of<br />
pressure, temperature and fuel–air equivalence ratio. For this reason, the atom ba<strong>la</strong>nce<br />
equations of the C–H–O–N system are consi<strong>de</strong>red along with the following eight<br />
equilibrium reactions (Ferguson, 1986):<br />
H + O ⇔ H O<br />
1<br />
2 2 2 2<br />
CO + O ⇔CO<br />
1<br />
2<br />
2 2<br />
CH + 2O ⇔ CO + 2H O<br />
4 2 2 2<br />
H + O ⇔OH<br />
1 1<br />
2 2 2 2<br />
O + N ⇔ NO<br />
1 1<br />
2 2 2 2<br />
(6.12)<br />
tel-00623090, version 1 - 13 Sep 2011<br />
1<br />
2<br />
1<br />
2<br />
1<br />
2<br />
H<br />
O<br />
N<br />
2<br />
2<br />
2<br />
⇔ H<br />
⇔ O<br />
⇔ N<br />
The various thermodynamic properties (specific enthalpy, specific internal energy,<br />
specific volume, specific heat capacity at constant pressure) and thermodynamic<br />
<strong>de</strong>rivatives (<strong>de</strong>rivative of logarithmic specific volume with respect to logarithmic<br />
temperature and pressure) of the unburned and burned mixtures, nee<strong>de</strong>d for the<br />
calcu<strong>la</strong>tions, are computed according to the mole fraction of each species and the gas<br />
mixture rule. For this purpose, the well established coefficients (Heywood, 1988) of the<br />
polynomial curves that have been fitted to the various species thermodynamic data<br />
from JANAF tables are used. For the evaluation of specific internal energy of species i,<br />
the following re<strong>la</strong>tion can be applied according to JANAF Table thermodynamic data<br />
(Gordon and McBri<strong>de</strong>, 1971; Heywood, 1988):<br />
5<br />
⎡⎛<br />
ain<br />
n ⎞ ⎤<br />
ui( T)<br />
= Rsi ⎢⎜<br />
∑ T ⎟+ ai6<br />
−T⎥<br />
⎣⎝<br />
n=<br />
1 n ⎠ ⎦<br />
(6.13)<br />
where constants a in for the above polynomial re<strong>la</strong>tion can be found, for example, in<br />
(Ferguson, 1986; Heywood, 1988). Two sets of data are avai<strong>la</strong>ble for constants a in , one<br />
for temperatures up to 1000 K and another for temperatures from 1000 to 5000 K. The<br />
reference temperature is 298 K. Also,<br />
h( T) = u ( T)<br />
+ R T<br />
(6.14)<br />
i i si<br />
171