Properties of Pure Substances. Pure Substance w A substance that has a fixed (homogeneous and...
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Transcript of Properties of Pure Substances. Pure Substance w A substance that has a fixed (homogeneous and...
Pure SubstancePure SubstancePure SubstancePure Substance A substance that has a fixed (homogeneous and invariable) chemical composition throughout is called a pure substance.
It may exist in more than one phase, but the chemical composition is the same in all phases.
Pure SubstancePure Substance Pure means “…of uniform and invariable
chemical composition (but more than one molecular type is allowed).” This allows air to be a pure substance.
All our substances will be pure. We will drop the use of the word. When we refer to a simple system we mean one filled with a pure substance--a simple, pure system.
Examples of Pure SubstanceExamples of Pure SubstanceExamples of Pure SubstanceExamples of Pure Substance
Water (solid, liquid, and vapor phases) Mixture of liquid water and water
vapor Carbon Dioxide Nitrogen Homogeneous mixture of gases, such as
air, as long as there is no change of phases.
Multiple phases mixture Multiple phases mixture of a Pure Substanceof a Pure Substance
vapor
liquid
vapor
liquid
Water Air
Pure OH 2
Not pure, different condensation temperatures for different components
Thermodynamic PropertiesThermodynamic Properties We have discussed extensive properties
such as m, U, and V (for volume) which depend on the size or extent of a system, and
Intensive properties such as u, v, T, and P (sometimes we write a “p” for pressure, using P and p interchangeably) which are independent of system extent.
Important Questions .….Important Questions .…. How many properties are needed to
define the state of a system? How do we obtain those properties?
Equation of StateEquation of State
Property TablesProperty Tables
Review - State PostulateReview - State Postulate The number of independent intensive
properties needed to characterize the state of a system is n+1 where n is the number of relevant quasiequilibrium work modes.
This is empirical, and is based on the experimental observation that there is one independent property for each way a system’s energy can be independently varied.
Simple systemSimple system A simple system is defined as one for
which only one quasiequilibrium work mode applies.
Simple compressible systems Simple elastic systems Simple magnetic systems Simple electrostatic systems, etc.
CompressibleCompressible
If we restrict our system to being compressible, we define what that quasiequilibrium work mode is:
PdV,W
Pdv
m
Vd P w
m
W
For a simple system,For a simple system, We may write P = P(v,T)
or v = v(P,T)
or perhaps T = T(P,v)
For a simple, pure substanceFor a simple, pure substance
y0 = y(y1,y2), or
P = P(v,T), v = v(P,T), and T = T(P,v)
What do these equations define, in space?
Equations used to relate properties are called “Equations of State”
Equation of StateEquation of State Any two independent, intrinsic properties are
sufficient to fix the intensive state of a simple substance.
One of the major task of Thermodynamics is to develop the equations of state which relate properties at a give state of a substance.
),(210 yyyy
Ideal gas “law” is a simple Ideal gas “law” is a simple equation of stateequation of state
RTPv
M
RR u
mRTPV
Ru = universal gas constant
= 8.3144 (kPa-m3)/(kgmol-K)
= 1.545 (ft-lbf)/(lbmol-R)
Phases of a Pure SubstancePhases of a Pure Substance
Solid phase -- molecules are arranged in a 3D pattern (lattice).
Liquid phase -- chunks of molecules float about each other, but maintain an orderly structure and relative positions within each chunk.
Gas phase -- random motion, high energy level.
Phase Equilibrium
p
heat
ice
p
liquid
ice
P = 1 atmT = -10 oC
liquid
p
liquid
p
vapor
p
vapor
P = 1 atmT = 0 oC
P = 1 atmT = 20 oC
P = 1 atmT = 100 oC
P = 1 atmT = 300 oC
Phase-change ProcessPhase-change Process
Compressed liquid -- not about to evaporate Saturated liquid -- about to evaporate Saturated liquid-vapor mixture --two phase Saturated Vapor -- about to condense Superheated Vapor -- not about to condense
T-v DiagramT-v Diagram
1Com
pres
sed
liqu
id
Saturated mixture
2
Supe
rhea
ted
vapo
r
Isobaric process P = 1 atm
34
5
v
T, Co
20
100
300
P-TP-T Diagram (Phase Diagram) Diagram (Phase Diagram) of Pure Substancesof Pure Substances
P-TP-T Diagram (Phase Diagram) Diagram (Phase Diagram) of Pure Substancesof Pure Substances
GAS @ gGAS
State d
W eight
LIQUID
GAS
W eight
LIQUID @ a
P
T
g
P
T
g
d
P
T
g
d
a
Superheated Vapor
Compressed Liquid
Isothermal ProcessIsothermal Process
P
T
bfa
P
T
b
Gas @ bGas @ b
Q
GAS
STATE f
LIQUID
Q
GASLIQUID
Q
P
T
bf
Superheated Vapor
Subcooled Liquid
Isobaric Process
a
Water Expands on Freezing!Water Expands on Freezing!
Ice floats on top of the water body (lakes, rivers, oceans, soft drinks, etc.).
If ice sinks to the bottom (contracts on freezing), the sun’s ray may never reach the bottom ice layers.
This will seriously disrupt marine life.
Saturation Temperature Saturation Temperature and Pressureand Pressure
Tsat -- Temperature at which a phase change takes place at a given pressure.
Psat -- Pressure at which a phase
change takes place at a given temperature.
Saturation TemperatureSaturation Temperature
Tsat = f (Psat)
p = 1atm = 101.3 kPa, T = 100 C
p = 500 kPa, T = 151.9 C
o
o
*T and P are dependent during phase change
*Allow us to control boiling temperature by controlling the pressure (i.e., pressure cooker).
Latent HeatLatent Heat Latent heat is the amount of energy
absorbed or released during phase change
Latent heat of fusion -- melting/freezing =333.7 kJ/kg for 1 atm H2O
Latent heat of vaporization --boiling/condensation =2257.1 kJ/kg for 1 atm H2O
P
v
Superheated region --substance is 100% vapor
Two-phase or saturation region -- gas
and liquid coexist
Subcooled or compressed liquid region
Satu
rate
d liq
uid
line
Saturated vapor line
Critical point
P-v DiagramP-v Diagram
P-v Diagram of a Pure P-v Diagram of a Pure SubstanceSubstance
P-v Diagram of a Pure P-v Diagram of a Pure SubstanceSubstance
SUPERHEATED
vIsothermal process
T-v Diagram of a T-v Diagram of a Pure SubstancePure Substance
T-v Diagram of a T-v Diagram of a Pure SubstancePure Substance
v
Critical & SupercriticalCritical & SupercriticalCritical & SupercriticalCritical & Supercritical The state beyond which there is no distinct
vaporization process is called the critical point.
At supercritical pressures, a substance gradually and uniformly expands from the liquid to vapor phase.
Above the critical point, the phase transition from liquid to vapor is no longer discrete.
Critical PointCritical Point Point at which the saturated vapor
and saturated liquid lines coincide. If T Tc or P Pc there is no clear
distinction between the superheated vapor region and the compressed liquid region.
Critical PointCritical Point A point beyond which T Tc and a
liquid-vapor transition is no longer possible at constant pressure. If T Tc , the substance cannot be liquefied, no matter how great the pressure.
Substances in this region are sometimes known as “fluids” rather than as vapors or liquids.
Vapor (Steam) DomeVapor (Steam) Dome The dome-shaped region encompassing the
two-phase, vapor-liquid equilibrium region. It is bordered by the saturated liquid line and
the saturated vapor line, both of which end at the triple line and end at the critical point.
The region below the vapor dome is also called: saturated liquid-vapor region, wet region, two-phase region, or saturation region.
Steam TablesSteam Tables Table A-1.1 Saturation water -- temperature table Table A-1.2 Saturation water -- pressure table Table A-1.3 Superheated vapor
P
v
saturation region
p=psat and T=Tsat
superheated region
If T=Tsat , ppsat
If p=psat , T>Tsat
Subcooled or
compressed
liquid region
If T=Tsat, ppsat
If p=psat,TTsat
For WaterFor Water
Two properties are not Two properties are not independent in the vapor dome independent in the vapor dome
(the two-phase region)(the two-phase region)
The temperature and pressure are uniquely related. Knowing a T defines the P and vice versa.
Use quality to determine the state in two-phase region.
Quality is related to the horizontal Quality is related to the horizontal differences of P-v and T-v Diagramsdifferences of P-v and T-v DiagramsQuality is related to the horizontal Quality is related to the horizontal
differences of P-v and T-v Diagramsdifferences of P-v and T-v Diagrams
QualityQualityQualityQuality In a saturated liquid-vapor mixture, the mass fraction
(not volume fraction) of the vapor phase is called the quality and is defined as
The quality may have values between 0 (saturated liquid) and 1 (saturated vapor). It has no meaning in the compressed liquid or superheated vapor regions.
mmm
mmm
mm
gf
g
vaporliquid
vapor
total
vaporx
What is v for something in the What is v for something in the two-phase region?two-phase region?
m
mvmv
m
V V
m
V v
vapgliqfvapliq
x1m
m;
m
mx
tot
liq
tot
vap
v = (1-x)vf + xvg = vf + x(vg - vf) = vf + xvfg
Enthalpy in Two-Phase RegionEnthalpy in Two-Phase Region
H = U + pV
h = u + pv
h = (1-x)hf + xhg = hf + x(hg - hf)
= hf + xhfg
Saturated MixtureSaturated MixtureSaturated MixtureSaturated Mixture In the saturated mixture region, the average value of any intensive property y is determined from
where f stands for saturated liquid and g for saturated vapor.
v = vf + x(vg - vf) = vf + xvfg
u = uf + x(ug - uf) = uf + xufg
h = hf + x(hg - hf) = hf + xhfg
s = sf + x(sg - sf) = sf + xsfg
Saturated MixtureSaturated Mixture
f : saturated liquidg : saturated vapor
TEAMPLAYTEAMPLAYComplete the table below as a team. The substance is water. Make sure everybody understands how to do it!
P (MPa) T(C) v(m3/kg) x (if appl.)
300 1.0
0.15 0.65
0.50 300
TEAMPLAYTEAMPLAYComplete the table below as a team. The substance is water. Use linear interpolation if needed.
P(MPa) T(C) u (kJ/kg) x (if appl.)
7.0 0.0
7.0 1.0
7.0 0.05
7.0 600
7.0 100
7.0 460