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Chemistry Praxis > Thermodynamics > Flashcards

Thermodynamics Flashcards

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
Q

First Law of Thermodynamics

A

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
Q

Second Law of Thermodynamics

A

in an isolated system the total entropy of the system increase with time (law of increased entropy)

27
Q

Entropy (S)

A

Often described as the measure of randomness or chaos within a system (number of possible configurations, or microstates)

28
Q

When will entropy increase?

A
  • 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
Q

Third Law of Thermodynamics

A

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
Q

Zeroth Law of Thermodynamics

A

Two objects are said to be in thermal equilibrium when they have the same temperature.

31
Q

Endothermic

A

Absorbs energy in the form of heat

32
Q

Endothermic reaction

A

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
Q

Examples of endothermic reactions

A
  • liquid water evaporation

- photosynthesis

34
Q

Exothermic process

A

Releases energy from the system into the environment

35
Q

Exothermic reaction

A

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
Q

Examples of exothermic reactions

A
  • Water vapor condensation (an exothermic process)

- hydrogen combustion (an exothermic reaction)

37
Q

Temperature

A

name given to the kinetic energy of all the atoms or molecules in a substance

38
Q

The more energy the atoms have…

A

the more they spin and vibrate & the higher the substance’s temperature.

39
Q

Heat

A

movement of energy from one substance to another

40
Q

How does energy flow?

A

Energy will spontaneously move from high-energy (high temp) substances to low energy (low temp) substances.

Think of phase changes.

41
Q

Heat capacity

A

(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
Q

Specific Heat

A

(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
Q

Phase Transition

A

When a substance changes from a solid, liquid, or gas phase to a different phase

44
Q

Condensing

A

gas to liquid

heat of vaporization (-)

45
Q

Evaporating

A

liquid to gas

heat of vaporization (+)

46
Q

Freezing

A

liquid to solid

heat of fusion (-)

47
Q

Melting

A

solid to liquid

heat of fusion (+)

48
Q

Deposition

A

Gas to solid

heat of sublimation (-)

49
Q

Sublimation

A

Solid to gas

heat of sublimation (+)

50
Q

Phase diagram

A

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
Q

Supercritical fluid

A

a state that has the properties of both liquid and gas

52
Q

Tm

A

melting point on a phase diagram that shows the temperature and pressure where the solid melts to a liquid

53
Q

Tb

A

boiling point/temperature and pressure at which liquid evaporates

54
Q

Two phase state

A

two phases coexist at the same time (ice melting)

55
Q

Triple point (T)

A

temperature and pressure where the solid, liquid, and gas states are in equilibrium

56
Q

Critical point (C)

A

temperature and pressure at which the substance becomes supercritical fluid

57
Q

Heat of vaporization (DeltaHvap)

A

energy needed to transform a liquid to a gas at constant pressure

58
Q

Heat of fusion

A

energy needed to transform a solid to liquid at constant pressure

59
Q

Heat of Sublimation

A

amount of energy needed to change a solid to gas without going through the liquid phase

60
Q

Molar heat

A

(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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