SINGLE PHASE A.C CIRCUITS ELECTRICAL ENGG SCIENCE CHAPTER - 6.
Chapter 4 Single-Phase System
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Transcript of Chapter 4 Single-Phase System
Chapter 4 Single Phase System
Material and Energy Balances
Single-Phase Systems
Liquid and Solid
Densities
Ideal gas relationships
Equation of States
(EOS) for Nonideal Gas
The Compressibility
Factor EOS
Topic OutcomesAt the end of Chapter 4, you should:• Describe the meaning of incompressible fluids, the
term "equation of state", ideal gas behavior, standard specific volume, partial pressure, compressibility factors, z and the critical T and P.
• Calculate PVT properties using ideal gas equation of states.
• Carry out PVT calculations for gas using truncated virial EOS, van der Waals EOS, SRK EOS and the compressibility factor EOS with either tabulated compressibility factors or a generalized compressibility chart for a single species and Kay's rule for non-ideal mixture of gases.
Introduction Before carried out a complete material balance, we
usually need to determine various physical properties of materials in order to derive additional relationship among the system variables.
3 way to obtain the values of physical properties (such as density, vapor pressure, solubility, heat capacity, etc)1. Handbook or database
- Perry’s Chemical Handbook, CRC Handbook of Chemistry & Physics, TRC Database in Chemistry & Engineering, etc
2. Estimation using empirical correlations3. Experimental work
Density of Liquid and Solid
Liquid and solid expanded during heating and density decreases. However, it is assumed that the densities are independent of temp.
Change in pressure also do not caused changes in solid and liquid densities. These substance is termed as incompressible.
2 methods to estimate the density of mixture consist n number of liquid. Method 1: Volume Additivity
Method 2: Average Pure Component Densities
n
i i
ix
1
1
n
iiix
1
Ideal Gases
Equation of state Equation that relates the molar quantity and
volume of a gas to temperature and pressure. Ideal gas equation of state
Simplest and most widely used for many engineering calculations involving gases at low pressure.
Used for gas a low pressure and high temperature. For high pressure and/or low temperature, more
complex equation of state for P,V and T calculation.
Ideal Gas Equation of State
From the assumptions that gas molecules: 1)have negligible volume, 2) no force on one another and 3) collide elastically with the wall container. The equation:
or
The use of this equation does not require to know the gas species:1 mol of an ideal gas at 0˚C and 1 atm occupies 22.415 liters, whether the gas is argon, nitrogen, mixture of propane and air, or any other single species or mixture of gases
nRTPV RTnVP
Ideal Gas Equation of State-cont.
P = absolute pressure
V = volume of the gas
n = number of moles of gas
R = gas constant which the unit depend on unit
of P, V, n, TT = absolute temperature
nRTPV
Ideal Gas Equation of State-cont.
Ideal gas equation of state can also be written as
Which ; specific molar volume of gas. Unit for gas constant, R
R= 83.14 cm3 bar mol-1 K-1 R= 8.314 J mol-1K-1
RTVP ˆ
nVV /ˆ
etemperaturmole
volumepressureRfor Unit
etemperaturmole
energyRfor Unit
Ideal Gas Equation of State-cont.
Density of ideal gas is calculated as:
Rule of thumb for when it is reasonable to assume ideal gas behavior:
Let Xideal be a quantity calculated using ideal gas equation of state (X can be pressure, volume, temperature or mole).
Error is estimated value is ε
RT
MP
V
M
ˆ
%100
true
trueideal
X
XX
V̂
To calculate is ideal specific molar volume,
If error calculated is satisfies this criterion, the ideal gas equation of state should yield an error less than 1%.
gasesother mole)-lb/ ft (320 L/mol 20
gasesdiatomicmole)lb/ ft (80L/mol 5ˆ%13
3
idealVif
Try YourselfExample 5.2-1
Standard Temperature and Pressure (STP)
A way to avoid the use of gas constant, R when using ideal gas equation
For ideal gas at arbitrary temperature, T and pressure, P
--------- (1) For the same ideal gas at standard reference
temperature, Ts and standard reference pressure, Ps (refer to STP).
-----------(2) Divide eq. 1 to eq. 2 gives
nRTPV
sss RTVP ˆ
sssT
Tn
VP
PV
ˆ
Standard Conditions for Gases
System Ts Ps Vs ns VsSI 273K 1atm 0.022415 m3 1 mol 22.4 m3/kmolcgs 273K 1atm 22.415 L 1 mol 22.4 L/molEnglish 492˚R 1atm 359.05ft3 1 lb-mole 359.05 ft3/lb-mole
Value of standard conditions (Ps, Ts, Vs) are known, above equation can be used to determine V for a given n or vice versa
Standard cubic meters (SCM) = m3 (STP) Standard cubic feet (SCF) = ft3 (STP) ^Vs= 22.4 m3 (STP)/kmol =22.4 L(STP)/mol=359 ft3 (STP)/lb-mole
Try YourselfExample 5.2-2
Try YourselfExample 5.2-3
Try YourselfExample 5.2-4
Ideal Gas Mixture
Suppose nA moles of species A, nB moles of species B, nc moles of species C and so on, is behave in ideal manner and contained in a volume, V at temperature, T and pressure, P.
Partial pressure, pA
The pressure that would be exerted by nA moles of species A alone in the same total volume, V at the same temperature, T of the mixture. Pyp AA
Ideal Gas Mixture The partial pressure of a component in an
ideal gas mixture is the mole fraction of that component times the total pressure.
The summation of partial pressure of the component of an ideal gas mixture is equal to total pressure (Dalton’s Law).
PPyyyppp CBACBA ....)(.....
Ideal Gas Mixture-cont.
Pure component volume, vA
The volume would be occupied by nA moles of A alone at the same total pressure, P and temperature, T of the mixture.
Amagat’s Law
Vyv AA
VVyyyvvv CBACBA ....)(.....
Volume fraction = vA/V; percentage by volume (%v/v)= (vA/V )x 100%
For an ideal gas mixture, the volume fraction is equal to the mole fraction of the substance:
70% v/v C2H6 = 70 mole% C2H6
Liquid acetone (C3H6O6) is fed at a rate of 400 L/min into a heated chamber, where it evaporates into a nitrogen stream. The gas leaving the heater is diluted by another nitrogen stream flowing at a measured rate of 419 m3 (STP) min. The combined gases are then compressed to a total pressure P= 6.3 atm gauge at temperature of 325˚C. the partial pressure of acetone ion this stream is pa=501 mmHg. Atmospheric pressure is 763 mmHg.
a) What is the molar composition of the stream leaving the compressor?
b) What is the volumetric flow rate of the N2 entering the evaporator if the temperature and pressure of this stream are 27˚C and 475 mmHg gauge?
Try This
Equation of State for Nonideal Gases
The ideal gas equation might be inaccurate for low pressure and high temp. conditions. Hence, more accurate equation will be introduced.
Either the ideal gas equation fits the PVT data for a species depends on system temperature and pressure which is critical temperature and critical pressure.
Critical temperature (Tc)- the highest temperature at which a species can exist in two phases (liquid and vapor), and the corresponding pressure is critical pressure (Pc).
Critical state- a substance at their critical temperature and critical pressure.
Gas vs Vapor
At pressure low enough for the species to not be a liquid:
Vapor: a gaseous species below its critical temperature.
Gas: a gaseous species above its critical temperature.
Species above Pc and above Tc- supercritical fluids.
Virial Equation of State Virial equation of state
B,C,D- second, third, fourth virial coefficients
Truncated virial equation
Tr=T/Tc ω – acentric factor from Table 5.3-1
Tc,Pc from Table B.1
....ˆˆˆ
1ˆ
32
V
D
V
C
V
B
RT
VP
V
B
RT
VPˆ
1ˆ
6.102.4110
422.0083.0;
172.0139.0);(
rrc
c
TB
TBBB
P
RTB
Try YourselfExample 5.3-1
Cubic Equations of State
Refer as cubic equation because when the equation is expanded, it become third-order equation for the specific volume.
To evaluate volume for a given temperature and pressure using cubic equation of state, we need to do trial and error procedure.
Two famous cubic equation of statea) Van der Waals equation of stateb) Soave-Redlich-Kwong (SRK) equation of state
Van der Waals Equation of State
(a/V2)- account for attractive force between moleculesb - correction accounting for the volume occupied by
the molecules themselves
2ˆˆ V
a
bV
RTP
c
c
c
c
P
RTb
P
TRa
864
27 22
Soave-Redlich-Kwong (SRK) Equation of state
)ˆ(ˆˆ bVV
a
bV
RTP
2
2
2
1561.055171.148508.0
)]1(1[/
086.40)(
42747.0
m
TmTTT
P
RTb
P
RTa
rcr
c
c
c
c
Try This
A gas cylinder with a volume of 2.5 m3 contains 1.00 kmol of carbon dioxide at T= 300 K. Use the Soave-Redlich-Kwong equation of state to estimate the gas pressure in atm.
Compressibility Factor Equation of State
orIf z=1, equation become ideal gas equation of state
The extent to which z differs from 1 is a measure of the gas is behaving nonideally.
Alternatively; can use generalized compressibility chart Figure 5.4-1 – generalized compressibility chart Fig. 5.4-2 to Fig. 5.4-4 – expansion on various
region in Fig. 5.4-1
zRTVP ˆRT
VPz
ˆ
Step to Use Read Compressibility Factor
1. Find Tc and Pc2. If gas is either Hydrogen or Helium, determine
adjusted critical temperature and pressure form Newton’s correction equation
3. Calculate reduce pressure and reduce temperature of the two known variables
4. Read of the compressibility factor from the chart c
cidealr RT
VPV
Pc
P
Tc
TTr
ˆ;Pr;
atmPPKTT cacc
ac 88
Class Discussion Example 5.4-2
Nonideal Gas Mixtures
Kay Rule: estimation of pseudocritical properties of mixture as simple average of pure a component critical constants
Pseudocritical temperature (Tc’)
Tc’= yATcA + yBTcB +……
Pseudocritical pressure (Pc’)
Pc’= yAPcA + yBPcB +……
Pseudocritical reduced temperature (Tr’)
Tr’= T/Tc’
Pseudocritical reduce pressure (Pr’)
Pr’= P/Pc’
Compressibility factor for gas mixture, zm
P
RTzV mˆ
A mixture of 75% H2 and 25% N2 (molar basis) is contained in a tank at 800 atm and -70°C. Estimate the specific volume of the mixture in L/mol using Kay’s rule.
The End