Hii
Given – the mass of ethanol burnt = 276 kg/h
Molar mass of ethanol = CH3CH2OH=(12+3+12+2+16+1)=46 g/mole
Mass flow rate of 512 kg/hr
Molar mass of oxygen =32 g/mole
Moles = Mass in gram /molar mass in gram/mole
=molar flow rate of ethanol = 276000/46=6000 moles /hr
Molar flow rate of oxygen = 512000/32=16000 moles/hr
Combustion reaction of ethanol
C2H5OH+ 3O2= 2CO2+3H2O selectivity 0.4
C2H5OH+ 2O2= 2CO+3H2O Selectivity = 0.6
As we are assuming complete combustion we can say that the moles of ethanol reacting via first and second process are 0.4:0.6
Assuming 1 hr of operation
C2H5OH+ 3O2= 2CO2+3H2O
Moles of C2H2OH reacted = 0.4*6000= 2400 moles
Moles of O2 reacted = 3*2400= 7200 moles
Moles of CO2 produced = 2*2400= 4800 moles
Moles of H2O produced =3*2400=7200 moles
C2H5OH+ 2O2= 2CO+3H2O
Moles of C2H2OH reacted = 0.6*6000= 3600 moles
Moles of O2 reacted = 2*3600= 7200 moles
Moles of CO produced = 2*3600= 7200 moles
Moles of H2O produced =3*3600=10800 moles
Total moles in the product
CO2=4800 moles
Molar flow rate = 4800*44=211.2 Kg/hr
CO= 7200 moles
Molar flow rate = 7200*28=201.66 kg/hr
H20=10800 moles +7200 moles = 18000 moles
Molar flow rate = 18000*18=324 kg/hr
Remaining O2= 16000-7200-7200=1600 moles
Molar flow rate = 1600*32=51.2 Kg/hr
Molar mass of CO2= 12+32= 44 g/mole
Molar mass of CO= 12+16= 28 g/mole
Molar mass of H20= 2+16= 18 g/mole
Also g/mole= kg/kmole ( 1 kg=1000 g,1 kmoles =1000 moles)
Input mass flow rate
Let us complete the table now
Compound |
Molar mass (kg/mole) |
Mass flow rate (Kg/hr) |
Molar flow rate (kmol/hr) |
C2H5OH |
46 |
276 input output-0 |
6 |
O2 |
32 |
512 input - 51.2 output |
16 input – 1.6 output |
CO2 |
44 |
211.2 |
4.8 |
CO |
28 |
201.66 |
7.2 |
H2O |
18 |
324 |
18 |
Total |
788 |
We can check the calculation here
Using law of conservation of mass
Mass in should be equal to mass out.
Mass in = 276+512 = 788 kg/hr
Mass out = 51.2+211.2+201.66+324= 787.5 kg/hr
We have taken some approximation while calculations so this little difference is coming.
Thank You
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