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ME 525 Example Problem:
Chemical Equilibrium Calculations
A rigid tank with a volume of 500 m
3
contains 65 kg of acetylene (C
2
H
2
), 128 kg
of oxygen (O
2
), and 140 kg of nitrogen (N
2
) at an initial temperature of 400 K.
The mixture is ignited, burns, and reaches chemical equilibrium.
The final
temperature is measured to be 2500 K.
Assume ideal gases, and note that the
O
2
/N
2
ratio is different from that of air.
The enthalpy of formation of C
2
H
2(g)
is
+226,730 kJ/kmol, and the constant pressure specific heat of C
2
H
2(g)
is 1.69
kJ/kgK.
The molecular weights for C
2
H
2
, O
2
, and N
2
are 26.0, 32.0, and 28.0
kg/kmol, respectively.
Assume that only CO
2
, H
2
O, H
2
, CO, and N
2
are present in
significant concentrations at state 2.
For the quadratic equation
2
0
ax
bx
c
,
the solution is
2
42
xb
b
a
c
a
.
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(a)
Calculate the initial and final pressures in the tank.
(Answers:
76.49 kPa,
520 kPa)
(b)
Calculate heat transfer
Q
12
to or from the tank.
(Answer: 1.13x10
6
kJ)
(c)
Calculate the concentration of O
2
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This note was uploaded on 04/17/2011 for the course ME 525 taught by Professor Lucth during the Spring '11 term at Purdue UniversityWest Lafayette.
 Spring '11
 Lucth
 Combustion

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