PPT 1

Question 1

What is a definite integral?

Answer 1

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

Question 2

What is energy?

Answer 2

the4 capacity to do work

Question 3

What are the two types of energy?

Answer 3

kinetic and potential

Question 4

What is an equation of state?

Answer 4

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

Question 5

What does R represent?

Answer 5

the universal gas constant

Question 6

What do the units of R depends on?

Answer 6

the values of P and V

Question 7

What are the units of PV

Answer 7

Joules

Question 8

What is a system?

Answer 8

the part of the universe that we are studying

Question 9

What are surroundings?

Answer 9

the rest of the universe

Question 10

What is a boundary?

Answer 10

the interface between systems and surroundings

Question 11

What is an open system?

Answer 11

can exchange both matter and energy with surroundings

Question 12

What is a closed system?

Answer 12

can exchange only energy with its surroundings

Question 13

What is an isolated system?

Answer 13

Can exchange neither matter nor energy with its surroundings

Question 14

What are macroscopic properties?

Answer 14

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

Question 15

What is an extensive property?

Answer 15

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

Question 16

Whta is an intensive property?

Answer 16

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

Question 17

What type of reation is always at equilibrium?

Answer 17

reversible

Question 18

What does isobaric mean?

Answer 18

constant pressure

Question 19

What does isothermal mean?

Answer 19

constant temperature

Question 20

What is an equation of state?

Answer 20

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

Question 21

Give an example of an equation of state?

Answer 21

ideal gas laws

Question 22

What is a state function?

Answer 22

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

Question 23

What are some examples of systems?

Answer 23

cells, organisms, macromolecules, DNA, RNA, proteins

Question 24

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

Answer 24

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

Question 25

What does the zeroth law define?

Answer 25

temperature

Question 26

What is the zeroth law?

Answer 26

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

Question 27

What is the zeroth law also known as?

Answer 27

thermal equilibrium

Question 28

What is a pratical application for the zeroth law?

Answer 28

thermometer

Question 29

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

Answer 29

directly proportional

Question 30

What is work?

Answer 30

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

Question 31

What is uniform motion?

Answer 31

atoms are being pushed in the same directionagainst an opposing force

Question 32

What type of work is uniform motion?

Answer 32

mechnical work

Question 33

What is a chemical example of uniform motion?

Answer 33

gas expansion or compression

Question 34

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

Answer 34

+ve

Question 35

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

Answer 35

-ve

Question 36

What is heat?

Answer 36

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

Question 37

What is random motion?

Answer 37

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

Question 38

what is a chemical example of random motion?

Answer 38

combustion of fuels

Question 39

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

Answer 39

+ve

Question 40

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

Answer 40

-ve

Question 41

Why quantify work?

Answer 41

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

Question 42

Why is quantifying work important?

Answer 42

for metabolical/biological processes

Question 43

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

Answer 43

-ve

Question 44

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

Answer 44

+ve

Question 45

What is the area under the PV graph equal to?

Answer 45

work

Question 46

When is there least expansion work?

Answer 46

when external pressure is equal to 0

Question 47

When is there maximum expansion work?

Answer 47

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

Question 48

What happens if Pext exceeds Pgas?

Answer 48

the gas will begin to compress

Question 49

What type of equilibrium is maintained between Pext and Pgas?

Answer 49

mechanical equilbirum

Question 50

How is pressure reversible?

Answer 50

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

Question 51

When does a system do maximum expansion work?

Answer 51

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

Question 52

Is work a state function? Why?

Answer 52

No, path matters

Question 53

Can work be different if delta V = 0?

Answer 53

yes, depends on path

Question 54

What is heat capacity?

Answer 54

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

Question 55

What does heat capacity depend on?

Answer 55

amount of a substance

Question 56

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

Answer 56

the change in temeprature

Question 57

Are temperaature and mean kinetic energy proportional?

Answer 57

yes

Question 58

What does KMT allow us to do?

Answer 58

define temperature in terms of molecular motion

Question 59

What is thermal motion?

Answer 59

random molecular motion that molecules undergo at T > 0

Question 60

What are the three assumptions of KMT?

Answer 60

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)

Question 61

What can we determine using KMT assumptions and Newtons laws?

Answer 61

pressure

Question 62

What is pressure the result of?

Answer 62

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

Question 63

What is the relationship between temperature and energy?

Answer 63

directly proportional (temerature depends on KE)

Question 64

What is the Boltzmann distribution?

Answer 64

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

Question 65

Do atoms and molecules have discrete or indiscreteamounts of energy?

Answer 65

discrete

Question 66

What are the four energy levels?

Answer 66

electronic, vibrational, rotational translational

Question 67

Which energy level has the largest gap between levels?

Answer 67

electronic

Question 68

Which energy level has the smallest gap between levels?

Answer 68

translational

Question 69

What does thermal motion ensure for energy levels?

Answer 69

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

Question 70

What is the order of vibrational energy levels?

Answer 70

kT

Question 71

What two factors control the ratio of the population?

Answer 71

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

Question 72

What happens to energy states as temperature increases?

Answer 72

the population distributes more

Question 73

Why do substances have different heat capacities?

Answer 73

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

Question 74

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

Answer 74

high

Question 75

What defines maximal work?

Answer 75

work done reversibly

Question 76

What is expansion work?

Answer 76

the work done when a system expands against an opposing pressure

Question 77

Is heat capacity an extensive or intensive property?

Answer 77

extensive

Question 78

Is specfic heat an extensive or intensive property?

Answer 78

intensive