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GEN CHEM - Q4 > ENTHALPY > Flashcards

ENTHALPY Flashcards

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1
Q

is the reaction with oxygen to produce small molecules such as CO2 and H2O

A

Combustion

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2
Q

liquid to solid

A

freezing

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3
Q

gas to liquid

A

condensation

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4
Q

gas to solid

A

deposition

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5
Q

Exothermic Processes

A

Combustion
Phase Changes: Freezing, Condensation, Deposition
Dissolution
Bond Formation
Electron Gain

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6
Q

two unstable atoms may form a stable molecule

A

Bond Formation

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7
Q

some ionic compounds that dissociate into ions in water release energy

A

Dissolution

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8
Q

electron affinity is the energy released when a gaseous atom accepts an electron

A

Electron Gain

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9
Q

these processes are accompanied by lowering of the temperature (cooling) of the surroundings

A

Endothermic Process

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10
Q

this can sometimes be endothermic

A

Dissolution

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11
Q

Endothermic Process

A
  • Phase Changes: Fusion, Vaporization, Sublimation
  • Bond Dissociation
  • Ionization
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12
Q

solid to liquid

A

fusion

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13
Q

liquid to gas

A

vaporization

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14
Q

solid to gas

A

sublimation

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15
Q

is the energy needed to break a bond joining two atoms

A

bind dissociation energy

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16
Q

is the energy needed to remove an electron from a gaseous atom

A

Ionization Energy

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17
Q

are process that release heat to surroundings

A

Exothermic processes

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18
Q

are processes that absorb heat from the surroundings

A

Endothermic Processes

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19
Q

is the sum of the internal energy (E) and the product of work at constant PRESSURE

A

Enthalpy

20
Q

is the expansion and compression of the system, therefore it is brought upon the change in PRESSURE and VOLUME

A

Work

21
Q

at constant pressure, enthalpy of a process is equal to the ________

A

Heat (q)

22
Q

is the difference between the enthalpies of product and enthalpies of reactants

A

enthalpy of reaction

23
Q

enthalpy change of solid to liquid

A

enthalpy of reaction
enthalpy of fusion

24
Q

enthalpy change of phase 1 to phase 2

A

enthalpy of translation

25
Q

enthalpy change of liquid to gas

A

enthalpy of vaporization

26
Q

enthalpy change of solid to gas

A

enthalpy of sublimation

27
Q

enthalpy change of solute to solution

A

enthalpy of solution

28
Q

enthalpy change of elements to compound

A

enthalpy of formation

29
Q

enthalpy change of compound

A

enthalpy of combustion

30
Q

delta H < 0 (negative value)

A

exothermic

31
Q

delta H > 0 (positive value)

A

endothermic

32
Q

is an extensive property (depends on the amount of substance involved in a process)

A

Enthalpy Change

33
Q

is the enthalpy change accompanying a process undergone by 1 mole of a substance

A

Molar Enthalpy Change

34
Q

is the physical state of a pure substance in its most stable form at 1 atm and 25 degrees celsius

A

thermodynamic standard state

35
Q

is the enthalpy change involved in the formation of 1 mole of a substance from elements in their standard states

A

standard enthalpy of formation of standard heat of formation

36
Q

is the enthalpy change involved in a chemical reaction at standard conditions (1 atm and 25 degrees celsius)

A

standard enthalpy of reaction of standard heat of reaction

37
Q

is it equal to the sum of the standard heats of formation of products less the sum of the standard heats of formation of reactants

A

standard enthalpy of reaction of standard heat of reaction

38
Q

is the sum of internal energy and the product of pressure and volume

A

enthalpy of a system

39
Q

is equal to heat at constant pressure. It gives us an idea whether the process is exothermic or endothermic

A

enthalpy of a process

40
Q

is a chemical equation that indicates the energy, particularly the heat of enthalpy change, that accompanies the reaction

A

thermochemical equation

41
Q

for an exothermic reaction, the sign of the standard heat of reaction is _________

A

negative

42
Q

for an endothermic reaction, the sign of the standard heat of reaction is ________

A

positive

43
Q

is the sum of the enthalpy changes of all steps leading to this reaction

A

enthalpy of a reaction

44
Q

change in enthalpy of a chemical reaction depends upon the initial and final state of a chemical reaction irrespective of the number of steps involved in a chemical reaction

A

Hess’s Law

45
Q

this law states that the enthalpy of a reaction is the sum of the enthalpy changes of the steps leading to this reaction

A

Hess Law

GEN CHEM - Q4 (3 decks)

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