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Chemistry > Test 13 > Flashcards

Test 13 Flashcards

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1
Q

The branch of science that studies the transfer of energy during chemical reactions or phase changes

A

Thermochemistry

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2
Q

Expresses the average kinetic energy in the particles of a sample

A

Temperature

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3
Q

An insulated container, similar to a thermos, in which a thermometer detects the enthalpy that occurs during a chemical reaction

A

Calorimeter

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4
Q

The heat that produces a phase change

A

Latent heat

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5
Q

The heat that produces a temperature change in the substance when applied

A

Sensible heat

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6
Q

Why do enthalpies of vaporization differ widely?

A

The strength of intermolecular attractions in different liquids vary

Higher value means stronger intermolecular attractions

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7
Q

The amount of thermal energy required to raise the temperature of 1 g of the substance by 1°C

A

Specific heat Csp

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8
Q

Substances with__specific heats require large amounts of energy for a given temperature change and will change temperature only slowly

A

High

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9
Q

Which retains heat longer, substances with high specific heat values or low specific heat values?

A

High specific heat values

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10
Q

Why do the products in an exothermic reaction have a lower enthalpy than the reactants

A

Because energy is released during the reaction

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11
Q

If the reaction is endothermic the energy will be a

A

Reactant

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12
Q

If the reaction is exothermic the energy will be a

A

Product

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13
Q

A negative enthalpy of reaction value signifies what kind of reaction?

A

Exothermic

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14
Q

The enthalpy of reaction of a reverse reaction has the__magnitude but the__sign of the delta H of the forward reaction

A

Same

Opposite

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15
Q

The enthalpy change for the reaction that produces one mole of a compound in its standard state from its elements in their standard states

A

Standard molar enthalpy of formation /\ H °f

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16
Q

What does the degree symbol of /\ H °f mean?

A

It signifies that this delta H refers to standard conditions

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17
Q

Energy released as heat by the complete burning of one mole of a substance at standard conditions

A

Standard molar enthalpy of combustion /\ H °c

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18
Q

r States that the enthalpy change of a reaction equals the sum of the enthalpy changes for each step of the process

A

Hess’s Law

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19
Q

What is always required to break bonds

A

Energy

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20
Q

Entropy measures

A

Randomness of a system

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21
Q

Entropy __as temperature increases

A

Increases

22
Q

Delta H represents

A

Enthalpy

23
Q

Delta S represents

A

Entropy

24
Q

What is the formula for calculating free energy change (/\ G)

A

/\G=/\H-T/\S

25
Q

What does a negative G indicate

A

A decline in free energy and it signifies that a reaction may occur spontaneously

The reaction is favorable

26
Q

J to KJ

A

Move decimal three places to the left

27
Q

KJ to J

A

move decimal three places to the right

28
Q

Must convert from

A

Celsius to Kelvin

29
Q

Formula for Celsius to Kelvin

A

°C + 273 = K

30
Q

Why does drink stay hot longer than pop tart

A

Water has a higher specific heat than a pop tart

31
Q

When determining free energy change the temperature must be in

A

K

32
Q

Symbol for free energy

A

G

33
Q

G measures

A

Favorability of reactions considering both entropy and enthalpy

34
Q

And spontaneous natural processes entropy tends to__and enthalpy __

A

Increases

Decreases

35
Q

If it’s going from weaker bonds to stronger bonds, it is

A

Exothermic

36
Q

Gas has the__entropy

A

Most

37
Q

Formula for /\H°reaction

A

/\H°reaction= E /\H products- E /\H reactants

38
Q

Formula for /\S°reaction

A

/\S°reaction= E /\S products- E /\S reactants

39
Q

Used to determine whether increase or decrease in entropy

A

Formula for /\S

40
Q

Formula for /\G

A

/\G= /\H- T /\S

41
Q

/\H- /\S+

A

/\G - always

42
Q

/\H- /\S-

A

/\G- at low temperatures

43
Q

/\H+ /\S+

A

/\G - at high temperatures

44
Q

/\H+ /\S-

A

/\G + always

45
Q

The measure of the dispersal of energy in a system; the net decrease of usable energy in the system for a given temperature and quantity of matter

A

Entropy S

46
Q

-/\H=

A

Exothermic

47
Q

+/\H=

A

Endothermic

48
Q

-/\S=

A

Decrease in entropy

49
Q

+/\S=

A

Increase in entropy

50
Q

The quantity of thermal energy required to convert one mole of a liquid at its boiling point to its vapor at the same temperature

A

Molar enthalpy of vaporization /\H vap

51
Q

A chemical equation that shows the reactants, products, and amount of energy that is released or absorbed as heat

A

Thermochemical equation

52
Q

Standard state

A

25°C (298 K), and one atm of pressure

Chemistry (32 decks)

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