Thermochemistry Flashcards

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

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
The heat given or absorbed within isochoric processes results in
Changes in internal energy
26
Isothermal processes are ones which occur at
Constant temperatures
27
Adiabatic processes are ones which occur when
No heat is exchanged between the systems and surroundings
28
In Adiabatic processes, the internal energy is equivalent to
Work
29
Hess's Law states that
Enthalpies are additive
30
Entropy is the measure of
Disorder in a system
31
Which phase has the most disorder?
Gas
32
Which phase has the least disorder?
Solid
33
Maximum entropy is accomplished at
Equilibrium
34
∆Suniverse equals to
∆S system + ∆S surroundings, equalling to 0
35
Entropy is a
State function
36
What are the three laws of Thermodynamics?
- Conservation of Energy - All spontaneous processes are ∆S system + ∆S surroundings > 0 - Entropy of perfectly crystalline substance at 0K is 0
37
Gibbs Free Energy communicates how
Changes in enthalpy and entropy affect reactions
38
What is the equation for Gibbs Free Energy?
∆G = ∆H - T∆S
39
What happens if ∆G is negative?
Reaction is spontaneous and moves forward
40
What happens if ∆G is positive?
Reaction is not spontaneous and moves in reverse
41
What happens if ∆G is 0?
System is in equilibrium
42
What does spontaneity indicate?
It reaction will occur
43
What happens when -∆H and -∆S?
Spontaneous at low temperatures
44
What happens when -∆H and +∆S?
Spontaneous at all temperatures
45
What happens when +∆H and +∆S?
Spontaneous at high temperatures
46
What happens when +∆H and -∆S?
Nonspontaneous at all temperatures
47
What is a process in which no heat is exchanged?
Isothermal