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CHEM 203 > PPT 1 > Flashcards

PPT 1 Flashcards

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1
Q

What is a definite integral?

A

integration of a function between two location divided into strips with infinitestimal width dx

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2
Q

What is energy?

A

the4 capacity to do work

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3
Q

What are the two types of energy?

A

kinetic and potential

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4
Q

What is an equation of state?

A

an expression that expresses obe variable (usually pressure) in terms of other variables in the system

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5
Q

What does R represent?

A

the universal gas constant

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6
Q

What do the units of R depends on?

A

the values of P and V

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7
Q

What are the units of PV

A

Joules

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8
Q

What is a system?

A

the part of the universe that we are studying

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9
Q

What are surroundings?

A

the rest of the universe

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10
Q

What is a boundary?

A

the interface between systems and surroundings

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11
Q

What is an open system?

A

can exchange both matter and energy with surroundings

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12
Q

What is a closed system?

A

can exchange only energy with its surroundings

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13
Q

What is an isolated system?

A

Can exchange neither matter nor energy with its surroundings

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14
Q

What are macroscopic properties?

A

define the state of a system (p, T, V, n, …)

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15
Q

What is an extensive property?

A

depend on the size of the system (n, m, V, area, …)

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16
Q

Whta is an intensive property?

A

independent of the size of the system (T, o, V/n, d, …)

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17
Q

What type of reation is always at equilibrium?

A

reversible

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18
Q

What does isobaric mean?

A

constant pressure

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19
Q

What does isothermal mean?

A

constant temperature

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20
Q

What is an equation of state?

A

connects two or more properties that describe the state of the system

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21
Q

Give an example of an equation of state?

A

ideal gas laws

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22
Q

What is a state function?

A

depends only on the4 state of the system and not on the path used to get to that state

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23
Q

What are some examples of systems?

A

cells, organisms, macromolecules, DNA, RNA, proteins

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24
Q

What does thermodynamics allow us to quantate about the energy of a system?

A
  1. how much energy we can harness from the system
  2. how much energy is exchanged in any process (metabolic, enzymatic…)
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25
Q

What does the zeroth law define?

A

temperature

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26
Q

What is the zeroth law?

A

when a hot object is placed in contact with a cold object, heat flows from the warmer to the cooler object until they are at the same temperature

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27
Q

What is the zeroth law also known as?

A

thermal equilibrium

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28
Q

What is a pratical application for the zeroth law?

A

thermometer

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29
Q

What is the relationship between temperature and volume when when pressure is constant?

A

directly proportional

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30
Q

What is work?

A

mode of transer of energy caused by motion against an opposing force

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31
Q

What is uniform motion?

A

atoms are being pushed in the same directionagainst an opposing force

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32
Q

What type of work is uniform motion?

A

mechnical work

33
Q

What is a chemical example of uniform motion?

A

gas expansion or compression

34
Q

When work is done on a system is it +ve or -ve?

A

+ve

35
Q

When a system does work is it +ve or -ve?

A

-ve

36
Q

What is heat?

A

mode of transfer of energy caused by temperature difference achieved by random motion of atoms or molecules

37
Q

What is random motion?

A

atoms and mnolecules in the cooler region oscillate/move around more rapidly and randomnly

38
Q

what is a chemical example of random motion?

A

combustion of fuels

39
Q

When heat is gained by a system is it +ve or -ve?

A

+ve

40
Q

When heat is lost by a system is it +ve or -ve?

A

-ve

41
Q

Why quantify work?

A

by measuring how much work a system can do, we can measure the energy stored in a system

42
Q

Why is quantifying work important?

A

for metabolical/biological processes

43
Q

Is work +ve or -ve when gas is exanding?

A

-ve

44
Q

Is work +ve or -ve when gas is compressing?

A

+ve

45
Q

What is the area under the PV graph equal to?

A

work

46
Q

When is there least expansion work?

A

when external pressure is equal to 0

47
Q

When is there maximum expansion work?

A

when the external pressure is at a maximum value (limited) –> when Pext is slightly lower than Pgas

48
Q

What happens if Pext exceeds Pgas?

A

the gas will begin to compress

49
Q

What type of equilibrium is maintained between Pext and Pgas?

A

mechanical equilbirum

50
Q

How is pressure reversible?

A

a slight change in pressure to inc Pext slightly more than Pgas will reverse the process (expansion to comprerssion)

51
Q

When does a system do maximum expansion work?

A

when it remains in mechanical equilibrium with its surroundings at all times

52
Q

Is work a state function? Why?

A

No, path matters

53
Q

Can work be different if delta V = 0?

A

yes, depends on path

54
Q

What is heat capacity?

A

for a system that undergoes a change in temeprature when heated, molar heat capacity determines what that change in temperature would be

55
Q

What does heat capacity depend on?

A

amount of a substance

56
Q

What do we need to know in order to calculate heat capacity?

A

the change in temeprature

57
Q

Are temperaature and mean kinetic energy proportional?

A

yes

58
Q

What does KMT allow us to do?

A

define temperature in terms of molecular motion

59
Q

What is thermal motion?

A

random molecular motion that molecules undergo at T > 0

60
Q

What are the three assumptions of KMT?

A
  1. Gases are composed of molecules that are in continuous motion, travelling in straight lines and changing direction only when they collide with other molecules of with the walls of a container (obey Newtons laws
  2. the molecules composing the gas are negligibly small compared to the distances between them. gas particles volume is zero
  3. gas moelcules exert no attraction or repulsice forces one each other or the container walls, their collisions are elastic (do not involve a loss of energy)
61
Q

What can we determine using KMT assumptions and Newtons laws?

A

pressure

62
Q

What is pressure the result of?

A

the microscopic collisions that these gas molecules have with the walls of the container

63
Q

What is the relationship between temperature and energy?

A

directly proportional (temerature depends on KE)

64
Q

What is the Boltzmann distribution?

A

describes the distribution os speeds among the particles in a sample of gas at a given temperature

65
Q

Do atoms and molecules have discrete or indiscreteamounts of energy?

A

discrete

66
Q

What are the four energy levels?

A

electronic, vibrational, rotational translational

67
Q

Which energy level has the largest gap between levels?

A

electronic

68
Q

Which energy level has the smallest gap between levels?

A

translational

69
Q

What does thermal motion ensure for energy levels?

A

that the molecules will be found spread over the energy levels available to them

70
Q

What is the order of vibrational energy levels?

A

kT

71
Q

What two factors control the ratio of the population?

A

1, difference in energy between two levels (higher gap = smaller ratio)
2. temperature (lower temperature = lower ratio)

72
Q

What happens to energy states as temperature increases?

A

the population distributes more

73
Q

Why do substances have different heat capacities?

A

depends on the distribution of energy levels:
- levels are close together = gain of energy through heat is a slight adjustment of the population, temperature does not hcnage significantly

74
Q

When a slight change in temperature required is it a high or low heat capacity?

A

high

75
Q

What defines maximal work?

A

work done reversibly

76
Q

What is expansion work?

A

the work done when a system expands against an opposing pressure

77
Q

Is heat capacity an extensive or intensive property?

A

extensive

78
Q

Is specfic heat an extensive or intensive property?

A

intensive

CHEM 203 (4 decks)

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