Steam Tabels
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Transcript of Steam Tabels
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What is Heat?
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What is Heat?
Heat is energy in transit.
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Units of Heat The SI unit is thejoule (J),
which is equal to Newton-metre (Nm).
Historically, heat was measured in terms of the ability
to raise the temperature of water.
The calorie (cal): amount of heat needed to raise thetemperature of 1 gramme of water by 1 C0 (from
14.50C to 15.50C)
In industry, the British thermal unit (Btu) is still used:amount of heat needed to raise the temperature of 1 lb
of water by 1 F0 (from 630F to 640F)
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Conversion between different
units of heat:
1 J = 0.2388 cal = 0.239x10-3 kcal = 60.189 Btu
1 cal = 4.186 J = 3.969 x 10-3 Btu
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Calculation of Sensible Heat
where T is the temperature change in the substance
Q = m c dTQ is the heat lost or gained by a substancem is the mass of substance
c is the specific heat of substance which changes with temperatureT is the temperature
When temperature changes causes negligible changes in c,
Q = m c dT = m c T
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Calculation of Sensible Heat
When temperature changes causes significant changes in c,
Q = m c T cannot be used.
Q = H = m h
Instead, we use the following equation:
where H is the enthalpy change in the substance
and h is the specific enthalpy change in the substance.
To apply the above equation, the system should
remain at constant pressure and the associated
volume change must be negligibly small.
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Calculation of Sensible Heat
Q = m c T (since c is taken as a constant)= (300 g) (0.896 J/g oC)(70 - 25)oC
= 12,096 J
= 13.1 kJ
Calculate the amount of heat required to raise the temperatureof 300 g Al from 25oC to 70oC.
Data: c = 0.896 J/g oC for Al
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Exchange of Heat
Heat lost by iron = Heat gained by water
(m c T)iron = (m c T)water
(100 g) (0.452 J/g oC)(80 - tf)oC
= (53.5 g) (4.186 J/go
C)(tf - 25)o
C80 - tf = 4.955 (tf-25)
tf = 34.2oC
Calculate the final temperature (tf), when 100 g iron at 80oC is
tossed into 53.5g of water at 25oC.
Data: c = 0.452 J/g oC for iron and 4.186 J/g oC for water
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Latent Heat
What is latent heat?
Latent heat is associated withphase change of matter
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Phases of Matter
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Phase Diagram: Water
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Phase Diagram: Water
Saturated steam
Superheated
steam
Saturated liquid
Compressed liquid
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Phase Diagram: WaterExplain why water is at liquid
state at atm pressure
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Phase Diagram: Carbon DioxideExplain why CO2 is at gas
state at atm pressure
Explain why CO2
cannot be made a
liquid at atm
pressure
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Latent Heat
Latent heat is the amount of heat added per unit mass of
substance during a phase change
Latent heat of fusion is the amount of heat added to melt
a unit mass of ice OR it is the amount of heat removedto freeze a unit mass of water.
Latent heat of vapourization is the amount of heat added
to vaporize a unit mass of water OR it is the amount ofheat removed to condense a unit mass of steam.
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Water:
Specific Heat Capacities and Latent Heats
Specific heat of ice 2.06 J/g K (assumed constant)
Heat of fusion for ice/water 334 J/g (assumed constant)
Specific heat of water 4.18 J/g K (assumed constant)
Latent heat of vaporization cannot be assumed a
constant since it changes significantly with the pressure,
and could be found from the Steam Table
How to evaluate the sensible heat gained (or lost) by
superheated steam?
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Water:
Specific Heat Capacities and Latent Heats
How to evaluate the sensible heat gained (or lost) bysuperheated steam?
Q = m c Tcannot be used since changes in c with changing
temperature is NOT negligible.
Q = H = m h
Instead, we use the following equation:
provided the system is at constant pressure and the
associated volume change is negligible.
Enthalpies could be referred from the Steam Table
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Properties of Steam
Learnt to refer to Steam Table to find properties of
steam such as saturated (or boiling point) temperatureand latent heat of vapourization at give pressures, and
enthalpies of superheated steam at various pressures and
temperatures.
)
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Warming curve for waterWhat is the amount of heat required to change 2 kg of ice
at -20o
C to steam at 150o
C at 2 bar pressure?
-20oC ice
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Warming curve for waterWhat is the amount of heat required to change 2 kg of ice
at -20o
C to steam at 150o
C at 2 bar pressure?
-20oC ice
0oC melting point of ice
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Warming curve for waterWhat is the amount of heat required to change 2 kg of ice
at -20o
C to steam at 150o
C at 2 bar pressure?
-20oC ice
0oC melting point of ice
120.2oC boiling point of water at 2 bar
Boiling point of water at 1 atm pressure is
100oC.
Boiling point of water at 2 bar is 120.2oC.
[Refer the Steam Table.]
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Warming curve for waterWhat is the amount of heat required to change 2 kg of ice
at -20o
C to steam at 150o
C at 2 bar pressure?
-20oC ice
0oC melting point of ice
120.2oC boiling point of water at 2 bar
150oC superheated steam
Specific heat
Specific heat
Specific heat
Latent heat
Latent heat
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Warming curve for waterWhat is the amount of heat required to change 2 kg of ice
at -20o
C to steam at 150o
C at 2 bar pressure?
Specific heat required to raise the temperature of ice from -20oCto 0oC
= (2 kg) (2.06 kJ/kg oC) [0 - (-20)]oC = 82.4 kJ
Latent heat required to turn ice into water at 0oC
= (2 kg) (334 kJ/kg) = 668 kJ
Specific heat required to raise the temperature of water from 0o
C to120.2oC
= (2 kg) (4.18 kJ/kg oC) [120.2 - 0)]oC = 1004.9 kJ
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Warming curve for waterWhat is the amount of heat required to change 2 kg of ice
at -20o
C to steam at 150o
C at 2 bar pressure?
Latent heat required to turn water into steam at 120.2oC and at 2 bar
= (2 kg) (2202 kJ/kg) = 4404 kJ
[Latent heat of vapourization at 2 bar is 2202 kJ/kg as could bereferred to from the Steam Table]
Specific heat required to raise the temperature of steam from 120.2oC
to 150oC
= (2 kg) (27702707) kJ/kg = 126 kJ
[Enthalpy at 120.2oC and 2 bar is the saturated steam enthalpy of
2707 kJ/kg and the enthalpy at 150oC and 2 bar is 2770 kJ/kg as
could be referred to from the Steam Table]
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Warming curve for waterWhat is the amount of heat required to change 2 kg of ice
at -20o
C to steam at 150o
C at 2 bar pressure?
Total amount of heat required
= 82.4 kJ + 668 kJ + 1004.9 kJ + 4404 kJ + 126 kJ
= 6285.3 kJ
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Application: Heat ExchangerIt is an industrial equipment in which heat is transferred from a hot
fluid (a liquid or a gas) to a cold fluid (another liquid or gas) without
the two fluids having to mix together or come into direct contact.
Hot fluid
at TH,in Hot fluid
at TH,out
Cold fluid
at TC,out
Cold fluid
at TC,in
Heat lost by the hot fluid
= Heat gained by the cold fluid
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Application: Heat Exchanger
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Heat Exchanger
mhot chot (TH,inTH,out) = mcold ccold (TC,outTC,in). .
Heat lost by the hot fluid = Heat gained by the cold fluid
mass flow rate
of hot fluid
Specific heatof hot fluid
mass flow rate
of cold fluid
Specific heatof cold fluid
Temperature
decrease in the
hot fluid
Temperature
increase in the
cold fluid
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Heat Exchanger
mhot chot (TH,inTH,out) = mcold ccold (TC,outTC,in). .
Heat lost by the hot fluid = Heat gained by the cold fluid
The above is true only under the following conditions:
(1) Heat exchanger is well insulated so that no heat is lost to the
environment
(2) There are no phase changes occurring within the heatexchanger.
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Heat Exchanger
Heat lost by the hot fluid = Heat gained by the cold fluid
+ Heat lost to the environment
If the heat exchanger is NOT well insulated, then
W k d E l 1 i H E h
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High pressure liquid water at 10 MPa (100 bar) and
30oC enters a series of heating tubes. Superheatedsteam at 1.5 MPa (15 bar) and 200oC is sprayed over
the tubes and allowed to condense. The condensed
steam turns into saturated water which leaves the
heat exchanger. The high pressure water is to be
heated up to 170oC. What is the mass of steam
required per unit mass of incoming liquid water?
The heat exchanger is assumed to be well insulated(adiabatic).
Worked Example 1 in Heat Exchanger
S l i W k d E l 1 i H E h
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Solution to Worked Example 1 in Heat Exchanger
S l i W k d E l 1 i H E h d
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High pressure (100 bar) water enters at 30oC and leaves at 198.3oC.
Boiling point of water at 100 bar is 311.0oC. Therefore, no phase
changes in the high pressure water that is getting heated up in the
heater.
Heat gained by high pressure water
= ccold (TC,out
TC,in)= (4.18 kJ/kg oC) x (170-30)oC
= 585.2 kJ/kg
[You could calculate the above by taking the difference in enthalpies at
the 2 given states from tables available.]
Solution to Worked Example 1 in Heat Exchanger contd.
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S l ti t W k d E l 1 i H t E h td
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Since there is no heat loss from the heater,
Heat lost by steam = Heat gained by high pressure water
Mass flow rate of steam x 1951 kJ/kg
= Mass flow rate of water x 585.2 kJ/kg
Mass flow rate of steam / Mass flow rate of water
= 585.2 / 1951= 0.30 kg stream / kg of water
Solution to Worked Example 1 in Heat Exchanger contd.
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Give the design of a heat exchanger
which has the most effective heat
transfer properties.
Assignment
Learning objectives:
1) To be able to appreciate heat transfer applications in pharmaceutical
industry
2) To become familiar with the working principles of various heatexchangers
3) To get a mental picture of different heat exchangers so that solving
heat transfer problems in class becomes more interesting
W k d E l 2 i H t E h
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Steam enters a heat exchanger at 10 bar and 200oC and
leaves it as saturated water at the same pressure. Feed-
water enters the heat exchanger at 25 bar and 80oC and
leaves at the same pressure and at a temperature 20oC
less than the exit temperature of the steam. Determine the
ratio of the mass flow rate of the steam to that of thefeed-water, neglecting heat losses from the heat
exchanger.
If the feed-water leaving the heat exchanger is fed
directly to a boiler to be converted to steam at 25 bar and300oC, find the heat required by the boiler per kg of feed-
water.
Worked Example 2 in Heat Exchanger
S l ti t W k d E l 2 i H t E h
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- Steam enters at 10 bar and 200oC and leaves it as saturated water at
the same pressure.
- Saturation temperature of water at 10 bar is 179.9oC.
- Feed-water enters the heat exchanger at 25 bar and 80oC and leaves
at the same pressure and at a temperature 20oC less than the exit
temperature of the steam, which is 179.9oC.
- Boiling point of water at 25 bar is (221.8+226.0)/2 = 223.9oC.- Therefore, no phase changes in the feed-water that is being heated.
Heat lost by steam = Heat gained by feed-water (with no heat losses)
Mass flow rate of steam x [28292778 + 2015] kJ/kg
= Mass flow rate of feed-water x [4.18 x (179.9-20-80) ] kJ/kg
Mass flow of steam / Mass flow of feed-water
= 333.98 / 2066 = 0.1617 kg stream / kg of water
Solution to Worked Example 2 in Heat Exchanger
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Use of Steam Tables
Saturated Vapor or Liquid
Liquid at Bubble-Point
Vapor at Dew-Point
Liquid and Vapor Co-existing
Superheated Vapor or Sub-Cooled Liquid
Vapor Above Dew-Point Temperature or Below Dew-
Point Pressure Liquid Below Bubble-Point Temperature or Above
Bubble-Point Pressure
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Vaporize 1kg Water at 20 C and Bubble Point Pressure
U Q W Q P V
m U Q mP V
Q m U P V
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Q U P V
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3 5
2
2403.0 83.91
57.8 0.0010021 0.0234 1 10
1,000
2454.3
Q m U P V
kJkgQ
kgmkg bar N kJ
kg m bar N m
Q kJ
H U PVH U P V
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Definitions
Degrees of Superheat
Difference between actual temperature and
saturation temperature at the same pressure Degrees of Sub-Cooling
Difference between actual temperature and the
saturation temperature at the same pressure.
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Vapor
Liquid
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Water Vapor Heating
1 kg from 100
o
C, 1 Bar to 200
o
C, 1 Bar
U Q W Q P V m U Q mP V
Q m U P V m H
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Water Vapor Heating
1 kg from 100
o
C, 1 Bar to 200
o
C, 1 Bar
2875 26761199
Q m U P V m H
kJkgQ kJ
kg
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Constant Volume Water Vapor Heating
1 kg from 100
o
C, 1 Bar to 200
o
C, P=?
0
V
U Q
m U Q
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Interpolation for Pressure
0
1
2
34
5
6
0.3 0.5 0.7 0.9 1.1 1.3 1.5 1.7 1.9 2.1 2.3
Specific Volume
Pressure
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Interpolation for Internal Energy
2640
2645
2650
2655
2660
0.3 0.5 0.7 0.9 1.1 1.3 1.5 1.7 1.9 2.1 2.3
Specific Volume
InternalEnergy
Linear Interpolation
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Linear Interpolation
1 1 2 2
2 1 2 1
2 1
2 1
1 1
1 1
1 1
2 1
1 1
2 1
y mx b
y mx b y mx by y m x x
y ym
x x
b y mx
y mx y mx
y y m x x
y yy y x x
x x
2 1 P P
P P V V
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2 1
1 1
2 1
2 1
1 1
2 1
5 11 1.69 2.17 2.10.425 2.17
2643 2658 2658 1.69 2.17 2654
0.425 2.17
1 2654 2507 147
Desired
Desired
P P V VV V
P bar
U U
U U V V V V
kJU
kg
kJQ m U kg kJ
kg