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1

kinetic energy

-energy that something has because it is moving

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2

Kinetic energy depends on a particle's...

mass and velocity

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3

translation

3D movement of particles

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4

movement of particles in a solid

vibration or rotation

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5

potential energy

energy something has as a result of its position

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6

types of potential energy

structural or positional

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7

examples of potential energy

gravitational, electrostatic, chemical bond energy

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8

-E =

q+w

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9

internal energy

sum of all the individual energies of nanoscale particles in a system

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10

internal energy depends on...

temperature, type, and number of particles

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11

higher T =

higher energy

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12

Joule

1 kg m^2/s^2

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13

calorie

original energy unit, 4.184 J

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14

calorie definition

energy required to heat one gram of water one degree celsius

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15

system

the region of the universe we are studying

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16

surroundings

everything else, separated from the system by a boundary

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17

open system

exchanges both energy and matter with the surroundings

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18

closed system

exchanges energy but mot matter with the surroundings

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19

isolated system

neither energy nor matter is exchanged between the system and surroundings

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20

open system example

a glass of soda

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21

closed system example

a unopened can of soda

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22

isolated system example

capped thermos bottle

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23

equation for calculating thermodynamic change

deltaE = Efinal -Einitial

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24

state variable

depends only on the state of the system and is independent of how it got there

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25

path variable

depends on how the state was reached

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26

heat (q)

the energy associated with the translation, rotation, and vibration of molecules

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27

magnitude of delta T depends on...

q

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28

molar heat capacity (C)

accounts for the identity of a material and is intrinsic

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29

molar heat capacity synonym

heat capacity

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30

heat capacity equation

C=q/n deltaT

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31

specific heat capacity

quantity of heat required to raise the temperature of one gram of a substance by one degree K

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32

specific heat synonym

specific heat

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33

work (w)

energy used to move an object against an opposing force

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34

work=

force x displacement

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35

work units

N*m

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36

expansion work

w= -Pext x deltaVsystem

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37

First Law of thermodynamics

deltaEsys = qsys + wsys qsurrounding = -qsystem

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38

automobile engine

some heat is lost while doing expansion work

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39

automobile engine equation

deltaEstove = qengine + wengine

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40

gas stove

all energy is converted into heat

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41

gas stove equation

deltaEstove = qstove

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42

calorimetry

device that measures heat flow in a chemical reaction

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43

calorimetry equation

qsys = qcalorimeter + qchemical = 0

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44

constant pressure calorimeter

-most common way to measure heat flow -used in most labs -explains biological systems -open system

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45

constant volume calorimeter

-bomb calorimeter used to counteract large pressure increase -closed system

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46

enthalpy equation

H = E + PV deltaH = deltaE + PdeltaV

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47

heat of formation

heat required to produce of a single product from standard elements in standard condition

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48

Hess's Law

the enthalpy change for any process s the sum of the enthalpy changes for any set of steps leading up to it

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49

enthalpy is related to

intermolecular force strength

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50

lattice energy

the energy required to separate one mole of an ionic solid

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51

exothermic reactions tend to favor

products

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52

free energy

energy we can use to do work

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53

energy is more likely to spread...

over many particles rather than a few

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54

entropy

a measure of dispersed energy of a system

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55

how can we disperse energy/matter?

spread something into a larger volume or allow two items to reach thermal equilibrium

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56

mixing of miscible substances

spontaneous

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57

most probable mixing pattern of particles

has the most uniform distribution of particles thru the volume the particles occupy

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58

W

number of energy equivalent arrangements of particles

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59

entropy is proportional to...

number of possible arrangements

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60

Boltzmann equation for entropy

S = k ln(W)

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61

accessible microstates

probable number of arrangements of particles at a particular T

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62

third law of thermodynamics

entropy of a pure, perfect crystal is zero at O K

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63

standard molar entropy

entropy of one mole of a substance at P= 1 barr and T=25 C

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64

which phase of matter has the greatest entropy

gases

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65

quantum theory of entropy

energy levels for gas motion get closer together when the volume expands, more energy levels become accessible at a given T, E will disperse more over these levels

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66

when a processes product favored?

when energy is dispersed from few to many levels

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67

Carnot entropy equation

S= Sf-Si = qrev/T

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68

reversible process

can be reversed by a slight change in condition

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69

entropy of solids

very small as particles are essentially fixed

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70

entropy of liquids

moderate entropy as particles slide past eachother

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71

entropy of gases

large entropy as particles move freely

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72

Factors that increase entropy

-greater motion -greater complexity -weaker ionic force -large matter dispersal -particle mass -temperature -dissolution

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73

entropy of aqueous solutions

tends to be large as it allows for a greater dispersion of ions

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74

less condensed phase is always...

more favorable

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75

spontaneous process

-occurs naturally under certain conditions -can be instantaneous or slow

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76

nonspontaneous process

driven by a continual input of energy from an external source

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77

thermodynamics

study of relationships between the energy and work associated with chemical and physical properties

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78

spontaneous processes often result in...

greater dispersal of energy or matter

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79

microstates

special configuration of all the locations and energies of the atoms or molecules in a system

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80

increase of microstates with number of particles

exponential

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81

second law of thermodynamics

all spontaneous changes cause an increase in the entropy of the universe

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82

second law of thermodynamics equation

deltaSuniv = deltaSsys + deltaSsurr

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83

standard entropy change

the total entropy of the products - the total entropy of the reactants

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84

the total entropy of the universe is continuously...

increasing

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85

standard entropy of surroundings =

-deltaH of the system/T

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86

Gibbs free energy

combines S and H to predict spontaneity

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87

Gibbs energy equation

G = H - TS (or changes of)

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88

delta G < 0

free energy decreases; product favored

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89

delta G > 0

free energy increases, reactant favored

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90

gibbs free energy of formation equation

G = sum(nGproducts) - sum(nGreactants)

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91

free energy of a system during a reaction

continuosly decreasing

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92

G = 0

reaction has reached its most stable state (equilibrium)

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93

H-, S+

product favored at all T

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94

H-, S-

product favored at low T

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95

H+, S+

product favored at high T

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96

H+, S-

not product favored

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97

when is the free energy greatest?

when only the reactants are present

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98

delta G = wsys =

-wmax

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99

3 steps of extracting free energy from nutrients

digestion, conversion of enzymes to acetyl coenzyme A, citric acid cycle

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100

digestion

large molecules are broken down into smaller ones

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