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Algebra > Thermo > Flashcards

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

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2
Q

“Father of Thermodynamics”.

A

Nicolas Sadi Carnot

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3
Q

The mass or region outside the system

A

Surrounding

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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

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5
Q
  • the surface that surrounds the control volume.
A

Control Surface

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6
Q
  • a quantity of matter having same chemical composition or homogenous.
A

Phase

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7
Q

is a system in which there is no transfer of matter across the boundary.

A

Closed system (control mass)

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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
A

Open system

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9
Q

is a system in which neither mass nor energy cross the boundaries and it is not influenced by the surroundings.

A

Isolated system

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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

A

Classical thermodynamics

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11
Q

is the branch of theories.
thermodynamics that includes the atomic and molecular
It is the microscopic approach of
thermodynamics.

A

Statistical thermodynamics

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12
Q

is the branch of theories.
thermodynamics that includes the atomic and molecular
It is the microscopic approach of
thermodynamics.

A

Statistical thermodynamics

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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

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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.
A

Chemical Thermodynamics

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15
Q
  • In this phase, the substance does not take the shape or volume of the container.
A

Solid

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16
Q
  • In this phase, the substance does not take the shape or volume of the container.
A

Solid

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17
Q

In this phase the liquid is non-saturated. Non-saturated means that it is not at is boiling point.

A

Subcooled liquid

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18
Q

In this phase the liquid is non-saturated. Non-saturated means that it is not at is boiling point.

A

Subcooled liquid

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19
Q
  • In this phase the liquid that can absorb as much heat as it can without vaporizing.
A

Saturated liquid

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20
Q
  • In this phase the liquid that can absorb as much heat as it can without vaporizing.
A

Saturated liquid

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21
Q
  • In this phase, the liquid and vapor co-exist with the same temperature and pressure.
A

Liquid-vapor mixture

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22
Q
  • In this phase, the vapor has absorbed more heat than necessary to vaporize
A

Saturated vapor

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23
Q
  • In this phase, the gas does not behave in accordance with the ideal gas
A

Real gas

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24
Q
  • In this phase, the gas does not behave in accordance with the ideal gas
A

Real gas

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25
Q
  • In this phase, two or more gases mixed together freely.
    Vapor/Gas
A

Gas mixtures

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26
Q
  • In this phase, two or more gases mixed together freely.
    Vapor/Gas
A

Gas mixtures

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27
Q
  • In this phase, the gas (a highly superheated vapor) behaves in accordance with the ideal gas law.
A

Ideal gas

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28
Q

a working substance whose chemical composition remains the same even if there is a change in phase.

A

Pure Substance -

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29
Q
  • refers to the physical condition of the working substance such as temperature, pressure, density, specific volume, specific gravity or relative density.
A

State Properties

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30
Q
  • refers to the physical condition of the working substance such as temperature, pressure, density, specific volume, specific gravity or relative density.
A

State Properties

31
Q
  • refers lo the measurement of diffusion within the working medium resulting from molecular
    activity,
    conductivities, etc.
A

Transport Properties

32
Q
  • refers lo the measurement of diffusion within the working medium resulting from molecular
    activity,
    conductivities, etc.
A

Transport Properties

33
Q
  • are properties which are size independent such density.
A
  1. Intensive Properties
34
Q
  • are properties which depend on the size or extent of the system. Mass, volume and total energy are examples of extensive properties.
A

Extensive Properties

35
Q
  • are properties which depend on the size or extent of the system. Mass, volume and total energy are examples of extensive properties.
A

Extensive Properties

36
Q
  • an indication or degree of hotness and coldness and therefore a measure of intensity of heat.
A

Temperature

37
Q

The Four Temperature Scales

A
  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
Q

is the temperature measured from absolute zero.

A

Absolute Temperature

39
Q

is the temperature measured from absolute zero.

A

Absolute Temperature

40
Q

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)

A

Absolute Zero

41
Q

Conversion formulas

A

F = 9/5 C+ 32
R = F + 460
c = 5/9 (F + 32)
К = С + 273

42
Q

Conversion formulas

A

F = 9/5 C+ 32
R = F + 460
c = 5/9 (F + 32)
К = С + 273

43
Q

Temperature interval is the difference between two temperature readings from the same scale, and the change in temperature through which the body is heated.

A

The Temperature Interval (Change)

44
Q
  • the force exerted per unit area.
45
Q
  • the true pressure measured above a perfect vacuum.
A

Absolute Pressure

46
Q
  • the true pressure measured above a perfect vacuum.
A

Absolute Pressure

47
Q

The pressure measured above perfect vacuum

A

Gage pressure

48
Q

The pressure measured above perfect vacuum

A

Gage pressure

49
Q

Pressure obtained from barometric reading

A

Atmospheric pressure

50
Q

Minimum pressure needed to liquify gas at its critical temperature

A

Critical pressure

51
Q

Mass per unit volume

A

Mass density

52
Q

Formula for mass density

53
Q

Weight per unit volume

A

Weight density

54
Q

Volume per unit mass

A

Specific volume

55
Q

Ratio of the density of a certain substance to the density of water

A

Specific gravity/ relative density

56
Q

Form of energy associated with the kinetic random motion of large number of molecules

57
Q

Form of energy associated with the kinetic random motion of large number of molecules

58
Q

The heat needed to change the temperature of a body without changing its phase

A

Sensible heat

59
Q
  • the heat needed by the body to change its phase without changing its temperature.
A

Latent heat

60
Q

Latent Heat of Fusion -
(b) Latent Heat of Vaporization -

A

Latent Heat of Fusion - solid to liquid.
(b) Latent Heat of Vaporization - liquid to gas.

61
Q
  • the term used to describe the process of changing solid to gas without passing the liquid state.
A

Sublimation

62
Q
  • the reverse of sublimation. It is the process of changing gas to solid without passing liquid state.
A

Deposition

63
Q
  • 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:
64
Q
  • the heat energy transferred to a substance at a constant pressure process.
65
Q
  • the heat energy transferred to a substance at a constant pressure process.
66
Q
  • 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
A

Internal Energy

67
Q

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.

A

2nd law of thermodynamics

68
Q

Energy cannot be created nor destroyed it can only be transformed from one form to another

A

1st law of thermodynamics

69
Q

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.

A

Kelvin-Planck Statement Applied to Heat Engine

70
Q

The total entropy of pure substances approaches zero as the absolute thermodynamic temperature approaches zero.

A

3rd law of thermodynamics

71
Q

The total entropy of pure substances approaches zero as the absolute thermodynamic temperature approaches zero.

A

3rd law of thermodynamics

72
Q

When any two bodies are in thermal equilibrium with the third body, they are in thermal equilibrium with each other.

A

Zeroth law of thermodynamics

73
Q

is a theoretically ideal gas which strictly follows Boyle’s law and Charles’ law of gases.

A

Ideal gas or perfect gas

Algebra (7 decks)

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