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Physics > Thermo > Flashcards

Thermo Flashcards

(52 cards)

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1
Q

Engine

A

A machine designed to convert one or more forms of energy into mechanical energy

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2
Q

Heat engine

A

A physical or theoretical device that converts thermal energy to mechanical output

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3
Q

Carnot heat engine

A

A hypothetical engine that operates on the reversible Carnot Cycle

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4
Q

The system

A

The part whose properties we are studying

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5
Q

Surroundings

A

Involve everything else outside or around the system

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6
Q

Boundary

A

What the system exchanges matter or energy across to interact with its surroudings

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7
Q

Isolated System

A

Neither matter nor energy can be exchanged

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8
Q

Closed system

A

Only energy can be exchanged

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9
Q

Open system

A

Both energy and matter can be exchanged

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10
Q

Diathermal

A

When a system may be influenced thermally

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11
Q

Conditions for thermodynamic equilibrium

A

-Mechanical equilibrium (constant pressure)
-Chemical equilibrium (constant particle concentration)
-Thermal equilibrium (constant temperature)

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12
Q

Extensive vs intensive

A

A state variable that depends on the physical size of the system vs one that is independent of the system’s size

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13
Q

Conditions for reversibility

A

-process can be reversed by an infinitesimal change in conditions
-quasistatic
-no hysteresis

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14
Q

Quasisatic

A

Carried out so slowly that every state the system passes through may be considered an equilibrium state

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15
Q

Hysteresis

A

When a process is reversed it does not retrace its previous path but follows a different one

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16
Q

Irreversible

A

When energy is permanently lost from the system due to dissipative forces such as friction

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17
Q

Common reversible processes

A

Isothermal, isochoric, isobaric, adiabatic

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18
Q

Isothermal

A

The temperature of the system remains constant

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19
Q

Isochoric

A

The volume of the system remains constant

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20
Q

Isobaric

A

The pressure of the system remains constant

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21
Q

Adiabatic (adiathermal)

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A

No heat is exchanged between the system and its surroundings

22
Q

Thermal equilibrium

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A

When there is no net heat flow between bodies after they have been in thermal contact with each other through a diathermal wall. They will have restricted value of their pressure/volume coordinate systems.

23
Q

The zeroth law

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A

If two systems are separately in thermal equilibrium with a third, then they must also be in thermal equilibrium with each other

24
Q

Work is positive when

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A

Work is done on the system of interest

25
Work is negative when
The system does work on the surroundings
26
Work
Energy transferred between a system and its surroundings when a force is applied over a distance or when the system undergoes a change in its external variables
27
Heat
An energy transfer that happens between a system and its surroundings due to temperature difference
28
First law
Energy is conserved and heat and work are both forms of energy. dU = dQ + dW
29
A small change of entropy of a system, dS , is defined as
The small change in heat flow per unit temperature into the system, provided the heat flow corresponds to a reversible process
30
Carnot cycle four steps
Isothermal expansion, adiabatic expansion, isothermal compression, adiabatic compression
31
Kelvin statement
No process is possible whose sole result is the complete conversion of heat into work
32
Clausius statement
No process is possible whose sole result is the transfer of heat from a colder to a hotter body
33
Second law
No process is possible where the total entropy of the universe decreases. The total change in entropy is always greater than or equal to zero
34
Carnots theorem
No engine operating between two given reservoirs can be more efficient than a carnot engine operating between the same two reservoirs
35
Isentropic process
A process that is both adiabatic and reversible
36
The second law- another version
The entropy of an isolated system tends to a maximum. As the universe of a whole is an isolated system, internal energy of universe is constant and entropy of universe can only increase, we are heading towards the heat death of the universe
37
Natural variables
when the property is made as a function of its natural variables all variables can be worked out
38
Enthalpy (equation)
H = U + PV
39
Helmholtz function
F = U - TS
40
Gibbs function
G = H - TS
41
Enthalpy defintion
Energy required to build a system from nothing
42
Latent heat
Amount of heat energy added to or removed from a substance without changing its temperature. The change in heat at constant pressure
43
The condition for spontaneous change in a conservative mechanical system tells us:
A change can occur spontaneously if the internal energy decreases when the change occurs at constant entropy and volumej
44
If the function of state can be determined as a function of its natural variables,
then the function will yield all the thermodynamic properties of the system
45
Chemical potential
The change in a systems energy when one particle is added at constant entropy and volume
46
Chemical potential in relation to Gibbs function
Gibbs function per particle (G/N)
47
Along a line of coexistence:
μ1 = μ2
48
Clausius-Clapeyron equation
Shows that the gradient of the phase boundary (for pressure vs temperature) is determined by the latent heat, the temperature and the difference in volume between the phases. Experimental evidence for this is also evidence for the second law of thermodynamics
49
At triple point chemical potential:
μgas = μliq = μsolid
50
Critical point
The end of the vapour-pressure curve where liquid gas coexistence is reached.
51
Supercritical drying
Process used to remove liquid from a material without causing surface tension damage, by avoiding the liquid-gas phase boundary. Instead of evaporating the liquid (which can collapse delicate structures), the liquid is brought above its critical point, where it becomes a supercritical fluid, and then gently vented as a gas
52
Freeze drying
A dehydration process where a material is frozen and then its ice is removed by sublimation.

Physics (5 decks)

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