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OAT Chem New Kap > Thermochemistry > Flashcards

Thermochemistry Flashcards

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1
Q

What does the first law state?

A

Energy can’t be created or destroyed

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2
Q

What is the equation of the internal energy of the system?

A

∆E = q+w

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3
Q

The work of a system =

A

-(P∆V), where P = pressure

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4
Q

What is ∆H?

A

Enthalpy

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5
Q

What is ∆H when Pressure is constant?

A

Gravity

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6
Q

What is it when a solid turns into a liquid?

A

Fusion / melting (+∆H)

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7
Q

What is it when liquid turns into a gas?

A

Vaporization / Boiling (+∆H)

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8
Q

What is it when a solid turns into a gas?

A

Sublimation (+∆H)

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9
Q

What is it when a gas turns into a liquid?

A

Condensation (-∆H)

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10
Q

What is it when a liquid turns into a solid?

A

Freezing (-∆H)

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11
Q

What is it when a gas turns into a solid?

A

Deposition (-∆H)

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12
Q

What are the types of systems found?

A
  • Isolated
  • Closed
  • Open
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13
Q

What is an isolated system?

A

One which can’t exchange energy or matter with the surroundings

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14
Q

What is a closed system?

A

One that can exchange energy but not matter

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15
Q

What is an open system?

A

One that can exchange both matter and energy with the surroundings

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16
Q

∆H is

A

Enthalpy

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17
Q

∆S is

A

Entropy

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18
Q

∆G is

A

Standard Free Energy

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19
Q

Internal energy is the sum of

A

KE, PE, and chemical energies

20
Q

Internal energy is

A

Constant

21
Q

How do you measure change in enthalpy?

A

∆H prod - ∆H react

22
Q

Isobaric processes are ones which occur at

A

Constant pressures

23
Q

The heat given or absorbed within isobaric processes results in

A

Changes in enthalpy

24
Q

Isochoric processes are ones which occur at

A

Constant volume

25
Q

The heat given or absorbed within isochoric processes results in

A

Changes in internal energy

26
Q

Isothermal processes are ones which occur at

A

Constant temperatures

27
Q

Adiabatic processes are ones which occur when

A

No heat is exchanged between the systems and surroundings

28
Q

In Adiabatic processes, the internal energy is equivalent to

A

Work

29
Q

Hess’s Law states that

A

Enthalpies are additive

30
Q

Entropy is the measure of

A

Disorder in a system

31
Q

Which phase has the most disorder?

A

Gas

32
Q

Which phase has the least disorder?

A

Solid

33
Q

Maximum entropy is accomplished at

A

Equilibrium

34
Q

∆Suniverse equals to

A

∆S system + ∆S surroundings, equalling to 0

35
Q

Entropy is a

A

State function

36
Q

What are the three laws of Thermodynamics?

A
  • Conservation of Energy
  • All spontaneous processes are ∆S system + ∆S surroundings > 0
  • Entropy of perfectly crystalline substance at 0K is 0
37
Q

Gibbs Free Energy communicates how

A

Changes in enthalpy and entropy affect reactions

38
Q

What is the equation for Gibbs Free Energy?

A

∆G = ∆H - T∆S

39
Q

What happens if ∆G is negative?

A

Reaction is spontaneous and moves forward

40
Q

What happens if ∆G is positive?

A

Reaction is not spontaneous and moves in reverse

41
Q

What happens if ∆G is 0?

A

System is in equilibrium

42
Q

What does spontaneity indicate?

A

It reaction will occur

43
Q

What happens when -∆H and -∆S?

A

Spontaneous at low temperatures

44
Q

What happens when -∆H and +∆S?

A

Spontaneous at all temperatures

45
Q

What happens when +∆H and +∆S?

A

Spontaneous at high temperatures

46
Q

What happens when +∆H and -∆S?

A

Nonspontaneous at all temperatures

47
Q

What is a process in which no heat is exchanged?

A

Isothermal

OAT Chem New Kap (17 decks)

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