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GLE 2024 (Day 3) > THERMODYNAMICS > Flashcards

THERMODYNAMICS Flashcards

1
Q

A porton of the universe which can be isolated physically or mentally in order to be studied

A

System

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2
Q

The adjacent portions of the universe outside such isolate entity being studied

A

Surroundings

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3
Q

Energy in Motion

A

Kinetic

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4
Q

Energy at Rest

A

Potential

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5
Q

Describes a configuration of minimum energy

A

Stable

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6
Q

Describes a configuration of maximum energy capable of spontaenous cange

A

unstable

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7
Q

Systems naturally (avoid, tend) configurations of min. energy

A

Tend to

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8
Q

State that is neither stable nor unstable

A

Metastable

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9
Q

the study of motion such as projectiles or falling rock

A

Mechanics

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10
Q

deals with the energy of heat and work

A

Thermodynamics

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11
Q

Measure of Energy transfer that occur when an object is moved over at as distance by external force

A

Work

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12
Q

Measure of Energy content/Driving force of chemical systems or Spontaneity of Reaction

A

Gibbs Free Energy

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13
Q

Mathematical Expression of Gibbs Free Energy

A

G = H - TS
(H-Enthalphy
T- emp in K
S - Entropy)

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14
Q

The measure of Heat Content of a system per unit mass volume
Internal Energy + (Volume*Pressure)

A

Enthalpy

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15
Q

The measure of thermal energy per unit temp unavailable for work or

measure of the molecular randomness of a system

A

Entropy

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16
Q

Between solid, Liquid and Gas, which has the greatest entropy?

A

Gas

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17
Q

Stable Systems have (Min, Max) Gibbs Free Enery

A

Minimum

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18
Q

If ?G > 0 (Positive)

A

Backward Reaction (Endergonic)
Reactant have lower total free energy than products

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19
Q

If ?G < 0 (Negative)

A

Forward Reaction (Exergonic)
Products have lower totral free energy than reacttans

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20
Q

Gibbs free energy of a mineral in reference state

A

0

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21
Q

A property that is dependent upon the QUANTITY of te material in the system

A

Extensive Variable

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22
Q

Independent upon the quantity

A

Intensive Variable

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23
Q

The amount of heat required to raise 1 mole of a the substance 1deg cel

A

Heat Capacity

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24
Q

Constant Temperatures

A

Isothermal

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25
Q

Constant Pressure

A

Isobaric

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26
Q

If ?G = 0

A

Sustem is in equilibrium and in a phase diagram lies in the equilibrium curve

27
Q

Principle stating that in any distrubance in a system in dynamic equilibrium, the system will react in a fashion to mitigate or counteract the change

If a chane is imposed on a system at equilbrium, the position of the equilibrium will shift in a direction that tends to resuce such change

A

Le Chatelier’s Principle

28
Q

An equation that gives the slope of the equilibrium curve in a binary phase diagram

A

Clapeyron Equation

29
Q

Temperature is proportional to Enthalpy and Entrophy
Pressure is inversely proportional to Volume

A

Solid Lowest Entalphy and Entropy
Lowest Molecular Volume
Gases highest

30
Q

If ?H < 0 (Entalphy is Negative)

A

Exothermic - Palabas ang Heat

31
Q

If ?H > 0 (Entalphy is Positive)

A

Endothermic - papasok ang heat

32
Q

If ?H < 0 , ?S > 0, the reaction is

A

Fowardm Spontaneous at all T

33
Q

When will reaction be non spontaneous at all T

A

if enthalpy is positive and entropy is negative

34
Q

If both Enthalpy and Entropy is positive

A

Reaction will be spontaneous at high T

35
Q

If both Enthalpy and Entropy is negatvie

A

Reaction will be spontaneous at low T

36
Q

Matter and Energy can Pass

A

Open

37
Q

Matter can’t but energy can pass

A

Closed

38
Q

Both Matter and Energy cant pass

A

Isolated

39
Q

Solid - Gas

A

Sublimation

40
Q

Gas - Solid

A

Deposition

41
Q

Gas - Plasma

A

Recombination

42
Q

Plasma - Gas

A

Ionization

43
Q

Liquid - Gas

A

Evaporation

44
Q

Gas - Liquid

A

Condensation

45
Q

Liquid - Solid

A

Freezing

46
Q

Solid - Liquid

A

Melting

47
Q

Gibss Phase Formula

A

F = C-P+2

48
Q

At what values of F will chemical reactions generally occur

A

F<2

49
Q

At what value of F will continuous reactions occur and take place over range of temp in constant pressure

A

F>0

50
Q

At what value of F will Discountinuous reaction occur and thus cannot involve compostional or temp changes and the entire reaction must occur at single temp

A

F=0

51
Q

Represents the mixture that has the lowest freezing Pt

A

Eutectic

52
Q

Represents the last solid to form when freezing

A

Eutectic

53
Q

weight loss that occurs when poweered sample is heate to about 800 deg cel at w/c pt all the remaining volatiles are released and is a quantitative indicator of secondary hydrous alteration

A

Loss of Ignition (LOI)

54
Q

Shows relative pressure at the time of melting and is useful in assessing silica saturation a.k.a Cation Norm

A

CIPW (Cross Iddings, pearson, Washington

55
Q

Volume % of the minerals seen

A

Mode

56
Q

Calculated Idealized Mineralization or
A set of hypothetical minerals that could crystallize from a magma with the same chemical composition as the rock

A

Norm

57
Q

MgO versus selected Major Oxide Elemens

A

Fenner Diagram

58
Q

SiO2 vs selceted Major Oxides and oldest Bivarate Diagram

A

Harker Diagram

59
Q

Alkali vs silica for Volcanic Rocks (X - SiO2 , Y - Na2O+K2O)

A

TAS

60
Q

Differentiate Ultramafics Komatiite and Picrite

A

Komatiite
>18% wt MgO
Has characteristicallY Spinifex Texture w/c implies veryvery fast cooling from very very hot magma
almost eclusively formed in Archaean

Picrite
Have lots of Olivine occurs as penocryst or xenocryst
15% wt MgO

61
Q

a diagram w/c further subdivides the subalkaline series into Tholeeitic and Calc Alkaline

A

AFM
A = Na2O+ K2O
F = FeO + Fe2O3
M = MgO

62
Q

Where would MORB plot in AFM?

A

Near tholeiitic siginifying Fe enrichemnt

63
Q

Calc alkaline are only found in

A

Subduction zones due to water conent which would change the sequence of crystallizing minerals and delays crystallization of Plagioclase

GLE 2024 (Day 3) (48 decks)

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