I just want to ask question about this as I'm not sure what I to do next:
The product gas from a combustion reaction has the following dry basis molar composition:
CO2 80.35%
CO 4.73%
SO2 0.03%
O2 14.89%
Pure oxygen is fed to the furnace in 10% excess of that required for complete combustion. There is no oxygen in the fuel (fixed or gaseous). Calculate the elemental composition of the fuel (mole % of elements C,H & S). Base calculations on 100 moles of dry outlet gas.
Take SO2 to be the fully combusted form of S.
Here is my working so far:
'O'in='O'out
2*'O2'in=2*'CO2'out+1*'CO'out+2*'SO2'out+2*'O2'out+1*'H2O'out
2*'O2'in=2*80.35+1*4.73+2*0.03+2*14.89+1*'H2O'out
'C'in='C'out
'C'in='CO2'out+'CO'out=80.35+4.73=85.08mols
'S'in='S'out
'S'in=1*'SO2'out=1*0.03=0.03mols
0.1=(O2feed-O2theoretical)/(O2theoretical)
Complete combustion
S+O2->SO2 0.03mols O2
C+O2->CO2 85.08mols O2
H2+1/2O2->H2O x mols O2
Incomplete Combustion
C+1/2O2->CO
The answer is
-
C 34.63%
H 65.36%
-
S 0.0122%
-
But the problem is that I do not know how to get to this answer. Please explain it to me step by step and/or the solution(maths/algebra behind it)
Thanks.
Edited by geo123, 15 April 2015 - 04:23 PM.