1. Pressure versus
temperature (P-T)
2. Pressure vs. volume (P-v)
3. Temperature vs. volume (T-v)
4. Temperature vs. entropy (T-s)
5. Enthalpy vs. entropy (h-s)
6. Pressure vs. enthalpy (P-h)
The term saturation temperature designates the
temperature at which vaporization takes place.
For water at 99.6 C the saturation pressure is 0.1 M Pa, and for water at
0.1 Mpa, the saturation temperature is 99.6 C.
If a substance exists as liquid at the saturation temperature and
pressure it is called saturated liquid.
If the temperature is of the liquid is lower than saturation temperature
at the existing pressure it is called sub-cooled liquid or compressed liquid.
1. When a substance exists as part liquid and part vapor at the saturation
temperature, its quality is defined as the ratio of the mass of vapor to the
total mass.
2. If a substance exists as vapor at the saturation temperature, it is
called a saturated vapor.
3. When the vapor is at a temperature greater than the saturation
temperature, it is said to exist as superheated vapor.
4. At the critical point, the saturated liquid and saturated vapor state are
identical.
5. At supercritical pressures, the substance is simply termed fluid rather
than liquid or vapor.
6. If the initial pressure at –200C is 0.260 kPa, heat transfer
results in increase of temperature to –100C. Ice passes directly
from the solid phase to vapor phase.
7. At the triple point (0.6113 kPa) and a temperature of –200C,
let heat transfer increase the temperature until it reaches 0.010C.
At this point, further heat transfer may cause some ice to become vapor and
some to become liquid. The three phases may be present simultaneously in
equilibrium.
Tables of thermodynamic properties of many
substances are available, and in general, all these have same form.
Steam
tables are selected because steam is used extensively in power plants and
industrial processes.
The steam tables provide the data of useful
thermodynamic properties like T, P, v, u, h and s for saturated liquid,
saturated vapor and superheated vapor.
Since
the properties like internal energy, enthalpy and entropy of a system cannot be
directly measured; they are related to change in the energy of the system.
Hence one can determine Δu, Δh,
Δs, but not the absolute values of these properties. Therefore it is
necessary to choose a reference state to which these properties are arbitrarily
assigned some numerical values.
For water, the triple point (T = 0.01o
C and P = 0.6113 kPa) is selected as the reference state, where the internal
energy and entropy of saturated liquid are assigned a zero value.
In the saturated steam tables, the properties of
saturated liquid that is in equilibrium with saturated vapor are presented.
During
phase transition, the pressure and temperature are not independent of each
other. If the temperature is specified, the pressure at which both phases
coexist in equilibrium is equal to the saturation pressure.
Hence, it is possible to choose either
temperature or pressure as the independent variable, to specify the state of
two-phase system.
Depending on whether the temperature or pressure
is used as the independent variable, the tables are called temperature or
pressure tables.
The two
phases- liquid and vapor can coexist in a state of equilibrium only up to the
critical point.
Therefore the listing of the thermodynamic properties of steam in
the saturated steam tables ends at the critical point (374.15o C and
212.2 bar).
If the steam exists in only one phase
(superheated steam), it is necessary to specify two independent variables,
pressure and temperature, for the complete specification of the state. In the
superheated steam tables, the properties- v, u, h, and s- are tabulated from
the saturation temperature to some temperature for a given pressure.
The thermodynamic properties of a liquid and
vapor mixture can be evaluated in terms of its quality. In particular, the
specific volume, specific internal energy, specific enthalpy and specific
entropy of a mixture of quality X are given by
v = (1-X)vf + Xvg, u =
(1-X)uf + Xug, h = (1-X)hf + Xhg =
hf + Xhfg, s = (1-X)sf + Xhg
where hfg = hg - hf
= latent hat of vaporization.
The
locus of all the saturated states gives the saturated liquid curve AC and the
locus of all the saturated vapor states gives the saturated vapor states gives
the saturated vapor states gives the saturated vapor curve BC.
The
point C represents the critical point. The difference between vg and
vf reduces as the pressure
is increased, and at the critical point vg = vf .
At the critical point, the two phases-liquid and
vapor- are indistinguishable.
The pressure-volume (P-V) diagram for a pure
substance is shown in Figure. The curves AC and BC represent the saturated
liquid curve and saturated vapor curve, respectively, and C is critical point.
The
area under the curve represents the two-phase region. Any point M in this
region is a mixture of saturated liquid (shown as f) and saturated vapor (g).
Mollier (h-s) Diagram
The h-s diagram was introduced by Richard
Mollier and was named after him.
It consists of a family of constant pressure
lines, constant temperature lines and constant volume lines plotted on enthalpy
versus entropy coordinates.
In the two-phase
region, the constant pressure and constant temperature lines coincide.