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Thermodynamics
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RAT 11
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Class Objectives
Be able to define:thermodynamicstemperature, pressure, density,
equilibrium, amount of substancestates of matter and define them in the
context of a phase diagramgas laws
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Thermodynamics
Thermodynamics:“Therme” meaning heat, and“Dynamics” meaning strength
Thermodynamics is the science of what is possible and impossible
Major limitation: Cannot predict how long the process takes (This is the subject of rate processes)
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Thermodynamic Properties
Temperature = “degree of hotness”
Rapidly moving molecules (atoms) have a high temperature
Slowly moving molecules (atoms) have a low temperatureHigh T Low T
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Thermodynamic Properties
Pressure - force per unit area
A
FP
F
A
Impact Weight
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Thermodynamic Properties
Density - mass per unit volume
V
M
High densityLow density
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Thermodynamic Properties
Amount of Substance – how much is there
………….………………...
1 2 3 12 144 6.022 × 1023
Dozen
Gross
Avogadro’s Number
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Pair Exercise 1
A cube of osmium measures 0.2 m on a side. It sits on a table. At the contact between the table and osmium, calculate the pressure (N/m2). Note: Densities may be found in Table
11.1 Foundations of Engineering
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States of Matter
Solid Liquid
Gas Plasma
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Pressure, Temperature, and State
Plasma
Gas
Vapor
Liquid
Solid
Ttriple Tcritical
Ptriple
Pcritical
Pressure
Temperature
Critical Point
TriplePoint
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Gas Laws
apply only to perfect (ideal) gases Boyle’s Law Charles’ Law Gay-Lussac’s Law Mole Proportionality Law
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Boyle’s Law
2
12
1 V
V
P
P
T = const n = const
P1
V1
P2
V2
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Charles’ Law
1
2
1
2
T
T
V
VT1
V1
T2
V2
P = const n = const
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Gay-Lussac’s Law
1
2
1
2
T
T
P
PT1
P1
T2
P2
V = const n = const
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Mole Proportionality Law
1
2
1
2
n
n
V
V
T = const P = const
n1
V1
n2
V2
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Perfect Gas Law
The physical observations described by the gas laws are summarized by the perfect gas law (a.k.a. ideal gas law)
PV = nRTP = absolute pressureV = volumen = number of molesR = universal gas constantT = absolute temperature
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Values for R
Rlbmol·
psia·ft
Rlbmol·
atm·ft
mol·K
atm·L
mol·K
Pa·m
o
3
o
3
3
73.10
7302.0
08205.0
314.8
Rlbmol·
Btu
Rlbmol·
ft·lb
mol·K
cal
mol·K
J
o
of
986.1
1545
987.1
314.8
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Pair Exercise 2
A balloon is filled with air to a pressure of 1.1 atm. The filled balloon has a diameter of 0.3 m.
A diver takes the balloon underwater to a depth where the pressure in the balloon is 2.3 atm.
If the temperature of the balloon does not change, what is the new diameter of the balloon?
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Energy
Energy is the capacity to do work, but work is a form of energy...
It is easier to think of energy as a scientific and engineering “unit of exchange”, much like money is a unit of exchange.
Example1 car = $20k1 house = $100k5 cars = 1 house
=
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Energy Equivalents
A case for nuclear power? 1 kg coal = 42,000,000 joules 1 kg uranium =
82,000,000,000,000 joules (82x1012)
1 kg uranium = 2,000,000 kg coal!!
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Heat
Heat is the energy flow resulting from a temperature difference.
NOTE: HEAT AND TEMPERATURE ARE NOT THE SAME!
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Example
T = 100oC
T = 0oC
Temperature Profile in Rod
HeatVibrating copper atom
Copper rod
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Work
Heat flows due to a temperature “driving force”
Work is the energy flow from any other driving force
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Types of Work
Work Driving Force
Mechanical Force (Physical)
Shaft work Torque
Hydraulic Pressure
Electric Voltage
Chemical Concentration
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Mechanical Work
F
Fx
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Mechanical Work
xF
xxF
xF
dxF
dxFW
xx
x
x
x
x
12
2
1
2
1
2
1
(assume F is not a function of x)
i.e., work is the area under the F vs. x curve
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PV Work (Hydraulic)
VP
xAA
F
xFW
x
P PFA
V
P = const
F
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Pair Exercise 3
An ideal gas is contained in a closed system. Under constant pressure, the container is compressed from V1 to V2 (volume). Derive the equation for work in terms of the universal gas constant and temperature.