Thermo Flashcards
1
Q
A branch of physical sciences that treats various phenomena of energy and the related properties of matter, especially of the laws of transformation of heat into other forms of energy and vice-versa.
A
Thermodynamics
2
Q
“Father of Thermodynamics”.
A
Nicolas Sadi Carnot
3
Q
The mass or region outside the system
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Surrounding
4
Q
the real or imaginary surface that separates the system from its surroundings. The boundary of a system can either be fixed or movable
A
Boundary
5
Q
- the surface that surrounds the control volume.
A
Control Surface
6
Q
- a quantity of matter having same chemical composition or homogenous.
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Phase
7
Q
is a system in which there is no transfer of matter across the boundary.
A
Closed system (control mass)
8
Q
- is a system in which there is a flow of matter through the boundary. It usually encloses the device that involves mass flow, such as: compressor, turbine, or nozzle
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Open system
9
Q
is a system in which neither mass nor energy cross the boundaries and it is not influenced by the surroundings.
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Isolated system
10
Q
is the branch of thermodynamics that is concerned with thermodynamic states and properties (energy, work and heat) and with the laws of thermodynamics without the atomic interpretation
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Classical thermodynamics
11
Q
is the branch of theories.
thermodynamics that includes the atomic and molecular
It is the microscopic approach of
thermodynamics.
A
Statistical thermodynamics
12
Q
is the branch of theories.
thermodynamics that includes the atomic and molecular
It is the microscopic approach of
thermodynamics.
A
Statistical thermodynamics
13
Q
- It is the branch of thermodynamics that is concerned with the study of the interrelation of heat with chemical reactions or with a physical change of state within the confines of the laws of thermodynamics.
A
Chemical Thermodynamics
14
Q
- It is the branch of thermodynamics that is concerned with the study of the interrelation of heat with chemical reactions or with a physical change of state within the confines of the laws of thermodynamics.
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Chemical Thermodynamics
15
Q
- In this phase, the substance does not take the shape or volume of the container.
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Solid
16
Q
- In this phase, the substance does not take the shape or volume of the container.
A
Solid
17
Q
In this phase the liquid is non-saturated. Non-saturated means that it is not at is boiling point.
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Subcooled liquid
18
Q
In this phase the liquid is non-saturated. Non-saturated means that it is not at is boiling point.
A
Subcooled liquid
19
Q
- In this phase the liquid that can absorb as much heat as it can without vaporizing.
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Saturated liquid
20
Q
- In this phase the liquid that can absorb as much heat as it can without vaporizing.
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Saturated liquid
21
Q
- In this phase, the liquid and vapor co-exist with the same temperature and pressure.
A
Liquid-vapor mixture
22
Q
- In this phase, the vapor has absorbed more heat than necessary to vaporize
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Saturated vapor
23
Q
- In this phase, the gas does not behave in accordance with the ideal gas
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Real gas
24
Q
- In this phase, the gas does not behave in accordance with the ideal gas
A
Real gas
25
- In this phase, two or more gases mixed together freely.
Vapor/Gas
Gas mixtures
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- In this phase, two or more gases mixed together freely.
Vapor/Gas
Gas mixtures
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- In this phase, the gas (a highly superheated vapor) behaves in accordance with the ideal gas law.
Ideal gas
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a working substance whose chemical composition remains the same even if there is a change in phase.
Pure Substance -
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- refers to the physical condition of the working substance such as temperature, pressure, density, specific volume, specific gravity or relative density.
State Properties
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- refers to the physical condition of the working substance such as temperature, pressure, density, specific volume, specific gravity or relative density.
State Properties
31
- refers lo the measurement of diffusion within the working medium resulting from molecular
activity,
conductivities, etc.
Transport Properties
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- refers lo the measurement of diffusion within the working medium resulting from molecular
activity,
conductivities, etc.
Transport Properties
33
- are properties which are size independent such density.
1. Intensive Properties
34
- are properties which depend on the size or extent of the system. Mass, volume and total energy are examples of extensive properties.
Extensive Properties
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- are properties which depend on the size or extent of the system. Mass, volume and total energy are examples of extensive properties.
Extensive Properties
36
- an indication or degree of hotness and coldness and therefore a measure of intensity of heat.
Temperature
37
The Four Temperature Scales
1. Celsius or Centigrade (named after the Swedish astronomer, Anders Celsius)
2. Fahrenheit (named
after German physicist Gabriel
Daniel Fahrenheit)
3. Kelvin (named after British scientist Lord Kelvin, also known as Sir William Thomson)
4. Rankine (named after William Macquom Rankine)
38
is the temperature measured from absolute zero.
Absolute Temperature
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is the temperature measured from absolute zero.
Absolute Temperature
40
is the temperature at which the molecules stop moving. The absolute zero is equivalent to 0 K (-
273.15°C) or 0°R (-460°F)
Absolute Zero
41
Conversion formulas
F = 9/5 C+ 32
R = F + 460
c = 5/9 (F + 32)
К = С + 273
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Conversion formulas
F = 9/5 C+ 32
R = F + 460
c = 5/9 (F + 32)
К = С + 273
43
Temperature interval is the difference between two temperature readings from the same scale, and the change in temperature through which the body is heated.
The Temperature Interval (Change)
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- the force exerted per unit area.
Pressure
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- the true pressure measured above a perfect vacuum.
Absolute Pressure
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- the true pressure measured above a perfect vacuum.
Absolute Pressure
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The pressure measured above perfect vacuum
Gage pressure
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The pressure measured above perfect vacuum
Gage pressure
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Pressure obtained from barometric reading
Atmospheric pressure
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Minimum pressure needed to liquify gas at its critical temperature
Critical pressure
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Mass per unit volume
Mass density
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Formula for mass density
P= m/v
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Weight per unit volume
Weight density
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Volume per unit mass
Specific volume
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Ratio of the density of a certain substance to the density of water
Specific gravity/ relative density
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Form of energy associated with the kinetic random motion of large number of molecules
Heat
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Form of energy associated with the kinetic random motion of large number of molecules
Heat
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The heat needed to change the temperature of a body without changing its phase
Sensible heat
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- the heat needed by the body to change its phase without changing its temperature.
Latent heat
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Latent Heat of Fusion -
(b) Latent Heat of Vaporization -
Latent Heat of Fusion - solid to liquid.
(b) Latent Heat of Vaporization - liquid to gas.
61
- the term used to describe the process of changing solid to gas without passing the liquid state.
Sublimation
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- the reverse of sublimation. It is the process of changing gas to solid without passing liquid state.
Deposition
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- the measure of the randomness of the molecules of a substance. This is one of the thermodynamic properties very much useful in the evaluation of thermodynamic processes. The following facts will help solve some thermodynamic-entropy problems:
Entropy
64
- the heat energy transferred to a substance at a constant pressure process.
Enthalpy
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- the heat energy transferred to a substance at a constant pressure process.
Enthalpy
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- the energy stored within the body, It is the sum of the kinetic energies of all its constituent
interaction among these particles.
particles plus the sum of all the potential energies of
H = U + PV
Internal Energy
67
Heat cannot be transferred from a cold body to a hot body without an input of work. It similarly states that heat cannot be converted 100% into work.
2nd law of thermodynamics
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Energy cannot be created nor destroyed it can only be transformed from one form to another
1st law of thermodynamics
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It is impossible to construct a heat engine which operates in a cycle and receives a given amount of heat from a high temperature body and does an equal amount of work.
Kelvin-Planck Statement Applied to Heat Engine
70
The total entropy of pure substances approaches zero as the absolute thermodynamic temperature approaches zero.
3rd law of thermodynamics
71
The total entropy of pure substances approaches zero as the absolute thermodynamic temperature approaches zero.
3rd law of thermodynamics
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When any two bodies are in thermal equilibrium with the third body, they are in thermal equilibrium with each other.
Zeroth law of thermodynamics
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is a theoretically ideal gas which strictly follows Boyle's law and Charles' law of gases.
Ideal gas or perfect gas
