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The underlying structure > Week 1- Thermodynamics > Flashcards

Week 1- Thermodynamics Flashcards

1
Q

What are the two sub-disciplines of thermodynamics?

A

Classical thermodynamics and statistical thermodynamics.

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2
Q

Describe classical thermodynamics:

A

Classical thermodynamics deals with bulks propertiens and consider the macroscopic properties of matter.

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3
Q

Describe statistical thermodynamics:

A

It also consider microscopic properties of matter and it refers to the probabilities of things happening at a molecular level.

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4
Q

What’s a system?

A

A system is anything contained within a boundary.

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5
Q

What are the 3 types of system?

A

1) Open system 2) Closed System 3) Isolated system

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6
Q

Describe open system:

A

Open system can exchange both energy and matter with the sorroundings

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7
Q

Describe closed system:

A

Closed system exchange only energy with the sorroundings.

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8
Q

Describe isolated system:

A

Isolated system cannot exchange either energy or matter with the sorroundings.

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9
Q

What’s sorrounding?

A

Sorrounding is everything else in contact with the system.

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10
Q

What’s energy?

A

Energy is the capacity to do a work.

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11
Q

What are the two types of energy?

A

1) Kinetic Energy 2) Potential Energy (Gravitational and chemical)

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12
Q

What’s potential chemical energy?

A

Energy stored in molecules by virtue of their bond.

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13
Q

What does bond formation do?

A

Bond formation release energy

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14
Q

What does bond breaking do?

A

Bond breaking consumes energy

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15
Q

What are the two ways by which energy can be transfered from the system to the sorrounding?

A

1)Heat 2) Work

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16
Q

What’s heat?

A

Heat is energy dispersed in a random motion

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17
Q

What’s work?

A

Work is energy dispersed as non random motion

18
Q

Describe the -1 law of thermodynamics:

A

Heat travels from hot to cold

19
Q

Describe the 0 law of thermodynamics:

A

If the body A is in thermal equilibrium with the body B and the body B is in thermal equilibrium with body C then the body A is in thermal equilibrium with the body C.

20
Q

What’s internal energy?

A

Internal energy is the total energy within a system

21
Q

Describe the 1st law of thermodynamics:

A

The internal energy of an isolated system is constant

22
Q

What does Enthalphy measures?

A

Enthalpy measures the energy change in a system.

23
Q

What’s energy change?

A

Energy change is the difference between the energy consumed by the breaking of bonds and the energy release by the formation of bonds.

24
Q

If ΔH is negative…

A

If ΔH is negative the reaction is exothermic, system loses energy and become more stable.

25
Q

If ΔH is positive…

A

If ΔH is positive the reaction is endothermic, the system acquire energy and become less stable.

26
Q

What are the properties of spontaneus reactions?

A

Spontaneus reaction occurs without the input of energy and once started they proceeds to completion.

27
Q

What is the property of non-spontaneus reactions?

A

Non-spontaneus reaction require energy to start and proceed.

28
Q

What does Entrhopy measures?

A

Enthropy measures the ways in which energy is distributed within a system.

29
Q

Describe the second law of thermodynamics:

A

The enthropy of an isolated system increase for any spontaneous change.

30
Q

If ΔS is positive…

A

The reaction is spontaneous and exothermic.

31
Q

What’s the tendency of ΔH?

A

ΔH tends to be negative due to the natural tendency to fall to lower energy state.

32
Q

What’s the tendency of ΔS?

A

ΔS tends to be positive due to random thermal motion at molecular level.

33
Q

What’s Gibbs free energy?

A

Gibbs free energy is the energy produced which is free to do work.

34
Q

If ΔG is positive….

A

The reaction is non-spontaneous.

35
Q

If ΔG is negative…

A

The reaction is spontaneous

36
Q

If ΔG=0

A

The reaction is at thermal equilibrium

37
Q

Describe the 3rd law of thermodynamics:

A

The entropy, S, of a perfect crystal at the absolute zero is 0.

38
Q

What’s Boltzman probability?

A

Is the probability that the system will have an enthalphy H at a specific temperature T.

39
Q

What is degenerancy?

A

Degenerancy (w) is the number of different way in which the system can adapt to the enthalpy.

40
Q

Describe chemical equilibrium:

A

Chemical equilibrium is reached when the rate of the forward reaction is equal to the rate of the reverse reaction.

41
Q

Describe dynamic equilibrium:

A

A dynamic equilibrium which can be described as the probability of molecule being at one state or another at any given time.

42
Q

Describe heat capacity:

A

Heat capacity is the quantity of heat energy (q) we need to add to the system in order to increase its temperature.

The underlying structure (13 decks)

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