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Thermodynamics > Lesson 1 and 2 > Flashcards

Lesson 1 and 2 Flashcards

1
Q

Thermodynamics

A

An energy science which deals with the relations among heat, work and properties of system which are in equilibrium.

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2
Q

Zeroth law

A

Deals with thermal equilibrium

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3
Q

The first law

A

Throws light on concept of internal energy

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4
Q

The second law

A

Indicates the limit of converting heat into work and introduces the principles of increase of entropy

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5
Q

The third law

A

Defines the absolute zero of entropy

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6
Q

System

A

Finite quantity of matter (mass) or prescribed region of space

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7
Q

Surroundings

A

Is the region outside the system and its exchange the matter (mass) and energy with it

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8
Q

Boundary

A

NAME?

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9
Q

Universe

A

System, boundary and surroundings together

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10
Q

Closed system

A

Exchanges energy but not matter with the environment

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11
Q

Open system

A

Can exchange both matter and energy with the environment

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12
Q

Isolated systems

A

Can exchange neither energy nor matter with the environment

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13
Q

Adiabatic system

A

Thermally insulated from its surroundings, it can however, exchange work with its surroundings

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14
Q

Independent variables

A

It is the variables that are needed to describe the state of the system and a complete thermodynamic description. -can be directly found

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15
Q

Dependent variable

A

These are variables can be determined by the independent variables -you need a formula

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16
Q

Intensive properties

A

Do not depend on the mass of the system

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17
Q

Extensive properties

A

These properties depend on the mass of the system

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18
Q

Thermal equilibrium

A

The temperature of the system does not change with time and has same value at all points of the system

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19
Q

Mechanical equilibrium

A

There are no unbalanced forces within the system or between the surroundings. The pressure in the system is same at all points and does not change with respect to time.

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20
Q

Chemical equilibrium

A

No chemical reaction takes place in the system and the chemical composition which is the same throughput the system does not vary with time

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21
Q

Adiabatic process

A

Thermally insulated from its surroundings. It can however, exchange work with its surroundings

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22
Q

Isothermal process

A

Is that the temperature is constant when the system transfer from one state to another

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23
Q

Isobaric process

A

Is the process that occurs at constant pressure

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24
Q

Isochoric process

A

Is the process that occurs at a fixed size (constant volume)

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25
Cyclic process
Is the process in which the system is transmitted through a series of changes so that eventually returns to its initial state
26
Reversible processes
Can be stopped at any stage and reversed so that the system and surroundings are exactly restored to their initial states
27
Irreversible process
A process in which they system and the surroundings do not return to their original condition once the process is initiated
28
Homogeneous system
A system which consists of a single phase
29
Heterogeneous system
A system which consists of two or more phases
30
Macroscopic approach
Needs a basic math formula
31
Microscopic approach
Needs a complicated math formula
32
State (or point) function
When two properties locate a point on the graph (co-ordinate axes) Examples: pressure, temperature and volume
33
Path function
Cannot be located by a graph by a point but are given by the area Example: heat and work
34
stored energy
May be in form of internal, chemical and potential energy
35
Is a general term for both types of energies; transition and stored
Energy
36
Heat and Work
Are a form of transition energy. These are the only forms in which energy can cross the boundaries of a system. Neither heat or work can exist as stored energy.
37
Work
Is said to be done when a force (F) moves through a distance (x)
38
Unit for work
Is joule (J). Joule= N*m
39
If the work is done by the system
Work output of the system= -W
40
Work is done on the system
Work input to the system= +W
41
Is something which only appears at the boundary, when a system changes due to a difference in temperature between the system and its surroundings
Heat (Q)
42
Heat received by the system
#NAME?
43
Heat rejected or given up by the system
#NAME?
44
Units of heat
Heat, like work is a transition energy. Therefore the unit of heat is the joule
45
Endothermic reactions
These reactions absorb heat or other forms of energy from their surroundings.
46
Exothermic reaction
These reactions release heat or other forms of energy into their surroundings.
47
What type of reaction is this?
Endothermic
48
What type of reaction is this?
Exothermic
49
Heat capacity
The amount of heat required to raise the temperature of an object by 1C.
50
Specific heat
The amount of energy required to raise the temperature of 1gram of the substance by 1C.
51
The unit for specific heat
(J/g c)
52
Thermometer
Used for measuring ordinary temperatures
53
Pyrometers
Used for measuring high temperatures
54
Temperature
Is a thermal state of a body which distinguishes a hot body from a cold body. The temperature of a body is proportional to the stored molecular energy (internal energy).
55
Freezing point
The temperature at which water and ice states of the substance are in equilibrium at atmospheric pressure
56
Boiling point
The temperature at which the water and vapor states of the substance are in equilibrium at atmospheric pressure
57
What is needed for heat transfer to place?
A difference in temperature between two objects
58
Conduction
Is the transfer of energy by direct contact
59
Convection
Is the movement of heat by a fluid state such as water or air
60
Radiation
Is the transfer of heat by electromagnetic waves
61
Zeroth law
If they are the same temperature, then they will be in thermal equilibrium
62

Thermodynamics (1 decks)

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