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Thermodynamics Flashcards

(60 cards)

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1
Q

Thermodynamics

A

The relationship between energy, work and heat

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2
Q

State functions

A

Have value that does not depend on the path taken by the process to reach its final state (example: mass, volume, pressure)

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3
Q

Path function/process function

A

A property that does depend on the path taken by the process

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4
Q

System

A

Part of the universe where the actual process takes place or where observations are made

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5
Q

Surroundings

A

Rest of the universe that does not include system.

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6
Q

Three types of systems

A

Open system
Closed system
Isolated system

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7
Q

Open system

A

exchange of energy or matter between the system and its surroundings is possible

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8
Q

Closed system

A

only exchange of energy between the system and its surroundings is possible; exchange of matter is not possible

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9
Q

Isolated system

A

No exchange of energy or matter between system and its surroundings is possible

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10
Q

Energy

A

Measured in Joules (J)

Property needed to perform work on or to heat an object

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11
Q

Kinetic energy

A

Energy possessed by objects in motion

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12
Q

Potential Energy

A

Energy possessed by objects that have the potential to be in motion due to their position.

Defined in relation to a specific point

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13
Q

Types of Kinetic Energy

A

thermal, sound, motion, radiant

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14
Q

Types of potential energy

A

Chemical, elastic, nuclear, gravitation, electrical

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15
Q

Thermal Energy

A

Energy possessed by an object due to the movement and vibration of atoms or molecules, which generate heat

Kinetic

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16
Q

Sound Energy

A

Energy associated with the vibration of an object because of a force and subsequent transference of energy through the object in a wave.

Kinetic

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17
Q

Motion

A

Energy ass. with the movement of an object

Kinetic

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18
Q

Radiant

A

Energy from the sun, or the energy possessed by vibrating particles is electromagnetic energy.

Kinetic

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19
Q

Chemcial

A

Energy that exists in the bonds between molecules and atoms

Potential

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20
Q

Elastic

A

Energy that is stored due to the deformation of an elastic object

Potential

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21
Q

Nuclear

A

Energy that is responsible for holding the nucleus of an atom together

Potential

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22
Q

Gravitational

A

Energy possessed by an object by the virtue of its height

Potential

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23
Q

Electrical

A

Energy that is stored in a battery

Potential

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24
Q

Law of Conservation of Energy

A

Total amount of energy remains constant and cannot be created or destroyed. Energy can be transformed from one form to another.

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25
First Law of Thermodynamics
change in energy for a closed system is the difference between the heat supplied to the system and the work done by the system on its surroundings
26
Second Law of Thermodynamics
in an isolated system the total entropy of the system increase with time (law of increased entropy)
27
Entropy (S)
Often described as the measure of randomness or chaos within a system (number of possible configurations, or microstates)
28
When will entropy increase?
- temp increases - volume increases - # of molecules in a system increases - a solid or liquid changes to a gas - a solid changes to a liquid - a solution forms from a solid
29
Third Law of Thermodynamics
entropy of a pure crystalline substance at absolute zero is 0. because all molecules in pure substance at 0 degrees K would have no energy and would be locked in place, meaning there is only one possible microstate
30
Zeroth Law of Thermodynamics
Two objects are said to be in thermal equilibrium when they have the same temperature.
31
Endothermic
Absorbs energy in the form of heat
32
Endothermic reaction
the energy required to break te existing bonds is greater than the energy released when the new bonds form Positive change in enthalpy (DeltaH) due to system gaining heat
33
Examples of endothermic reactions
- liquid water evaporation | - photosynthesis
34
Exothermic process
Releases energy from the system into the environment
35
Exothermic reaction
Occurs when the energy required to break bonds is less than the energy released when new bonds form Negative change in enthalpy (-DeltaH) because the system is losing heat
36
Examples of exothermic reactions
- Water vapor condensation (an exothermic process) | - hydrogen combustion (an exothermic reaction)
37
Temperature
name given to the kinetic energy of all the atoms or molecules in a substance
38
The more energy the atoms have...
the more they spin and vibrate & the higher the substance's temperature.
39
Heat
movement of energy from one substance to another
40
How does energy flow?
Energy will spontaneously move from high-energy (high temp) substances to low energy (low temp) substances. Think of phase changes.
41
Heat capacity
(C) The amount of energy required to raise the temperature of a substance by 1K or 1C. The unit for measuring specific heat is JdegC or JK-1
42
Specific Heat
(c) the amount of energy needed to increase the temperature of a unit mass of a sample by 1 K or 1 deg C
43
Phase Transition
When a substance changes from a solid, liquid, or gas phase to a different phase
44
Condensing
gas to liquid heat of vaporization (-)
45
Evaporating
liquid to gas heat of vaporization (+)
46
Freezing
liquid to solid heat of fusion (-)
47
Melting
solid to liquid heat of fusion (+)
48
Deposition
Gas to solid heat of sublimation (-)
49
Sublimation
Solid to gas heat of sublimation (+)
50
Phase diagram
Shows the effect of temperature and pressure on a substance. Each element and compound has a unique phase diagram for them x-axis temp y-axis pressure
51
Supercritical fluid
a state that has the properties of both liquid and gas
52
Tm
melting point on a phase diagram that shows the temperature and pressure where the solid melts to a liquid
53
Tb
boiling point/temperature and pressure at which liquid evaporates
54
Two phase state
two phases coexist at the same time (ice melting)
55
Triple point (T)
temperature and pressure where the solid, liquid, and gas states are in equilibrium
56
Critical point (C)
temperature and pressure at which the substance becomes supercritical fluid
57
Heat of vaporization (DeltaHvap)
energy needed to transform a liquid to a gas at constant pressure
58
Heat of fusion
energy needed to transform a solid to liquid at constant pressure
59
Heat of Sublimation
amount of energy needed to change a solid to gas without going through the liquid phase
60
Molar heat
(of vaporization, fusion, and sublimation) is the amount of energy needed to change the substance between the relevant states

Chemistry Praxis (2 decks)

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