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The gas that comes out of a gasoline stabilizer has the following composition by volume: C3H8...

The gas that comes out of a gasoline stabilizer has the following composition by volume: C3H8 8%, CH4 78%, C2H6 10%, and C4H10 4%. This gas that comes out at 90 ° F and 16 psi of absolute pressure is supplied at the rate of 70,000 ft3 / h to a gas conversion plant, where the following reactions take place:


CnH2n + 2 + n H2O n CO + (2n + 1) H2

CO + H2O CO2 + H2.

CnH2n + 2 gases are converted to 95% and 90% of CO that also reacts, depending on the reactions. Make a process diagram and calculate:

a) Average molecular weight of the gas coming out of stabilizer.

b) Weight of the gas supplied to the conversion plant in lb / h.

c) Weight of the H2 that leaves the converter plate in lb / h.

d) Composition in volume of the gases that leave the converter plant.

Thank you!

Solutions

Expert Solution

Feed composition

C​​​​​​3​​H8    - 8%

CH​​​​​​​4 -  78%

C​​​​​​2 H​​6. -  10%

C​​​​​​4 H​​​​​​10 - 4%

M.W of propane = 3(12)+(8)= 44

M.W of methane = 12+4 = 16

M.W of ethane = 2(12)+6 = 30

M.W of butane = 4(12)+10 = 58

M.W(avg)= 44(0.08)+ 16(0.78)+ 30(0.10) + 58(0.04)= 21.32

B)

V = 70000 ft​​​​​3/h = 1982.1792 m​​​​​​3/h

T = 90°F = 32.22°C = 305.372 K

P = 16 psi

1 psi = 6894.757 Pa

16 psi = 110316.112 Pa

n = PV/(RT)

n = (110316.112×1982.1792)/(8.314×305.372)

n = 86127.658 mol/h = 86.12765 Kmol/h

Feed analysis

Component mol% Kmol/h M.W(Kg/Kmol) kg/h.
Propane 8 6.8902 44 303.168
Methane 78 67.1795 16 1074.872
Ethane 10 8.6127 30 258.381
Butane 4 3.4451 58 199.8158
Total 100 86.12765 1836.2368

Mass flow rate of gas = 1836.2368 Kg/h

1 Kg = 2.205 lb

Mass flow rate of gas = 4048.9021 lb/h

C)

The reactions occurring are

Conversion is 95%

Conversion of CO - 90%

Moles of H2 produced

= (6.8902((2×3)+1) + 67.1795((2×1)+1)+ 8.6127((2×4)+1)+ 3.4451 ((2×2)+1)))(0.95)= 327.2842 Kmol/h

M.w of H2 = 2 Kg/Kmol

Mass of H2 produced = 327.2842(2)=

654.5684 Kg/h

1 Kg = 2.205 lb

Mass of H2 produced = 654.5684(2.205)= 1443.323 lb/h

Moles of CO produced =( 6.8902(3)+ 67.1795(1)+8.6127(2) + 3.4451(4))(0.95)= 112.9131 Kmol/h

90% of CO reacts

D)

Composition of outlet gases

mol% = vol%

Component Kmol/h mol%
Propane 6.8902(0.05)= 0.34451 0.0775
Methane (67.1795)0.05)= 3.3589 0.7562
Ethane 8.6127(0.05)= 0.430635 0.0969
Butane 3.4451(0.05)= 0.17225 0.03878
CO 11.2913 2.542
CO2 101.6217 22.879
H2 327.2842 73.686
Total 444.158 100

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