Biomedical Engineering Reference
In-Depth Information
The volume fraction of a gas can be found by noting that the volume that
1 kmol of any gas occupies at normal temperature and pressure (NTP) (at 0
C
and 1 atm)
is 22.4 m
3
. So,
taking the example of hydrogen,
the volume of
1 kmol of hydrogen in the gas mixture is 22.4 nm
3
at NTP.
The total volume of the gas mixture is V
summation of volumes of all con-
5
5
P
([number of moles (n
i
)
22.4])/nm
3
stituting gases in the mixture
22.4n.
The volume fraction of hydrogen in the mixture is volume of hydrogen/total
volume of the mixture:
3
5
22
:
4n
H
n
h
n
5
4
P
n
i
5
V
H
x
H
(iv)
5
22
:
Thus, we note that:
mole fraction
The partial pressure of a gas is the pressure it exerts if it occupies the entire
mixture volume V. Ideal gas law gives the partial pressure of a gas component,
i,as
Volume fraction
5
n
i
RT
V
P
i
5
P
a
The total pressure, P, of the gas mixture containing total moles, n,is
n
RT
V
P
5
So we can write:
n
i
n
5
p
i
p
5
v
i
V
x
i
(v)
5
Partial pressure as fraction of total pressure
mole fraction
volume fraction.
5
5
x
H
P.
The molecular weight of the mixture gas, MW
m
, is known from the mass
fraction and the molecular weight of individual gas species
The partial pressure of hydrogen is P
H
5
X
MW
m
½
x
i
MW
i
(vi)
5
where MW
i
is the molecular weight of gas component i with mole fraction x
i
.
SYMBOLS AND NOMENCLATURE
ASH
weight percentage of ash (%)
C
weight percentage of carbon (%)
C
p
specific heat of biomass (J/g K)
specific heat of biomass at temperature
θ
C (J/g C)
C
p
θ
C
w
specific heat of water (J/g K)
d
pore
pore diameter (m)
e
rad
emissivity in the pores (
)
FC
weight percentage of fixed carbon (%)
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