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Chem/Phys EXAM 2 > Chapter 4 > Flashcards

Chapter 4 Flashcards

Work, Energy & Power

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1
Q

Forces can be used to do

A

Work

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2
Q

Force does work when it

A

Acts on an object & displaces the object in the direction of the force

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3
Q

What is the equation for work?

A

W=F (magnitude of force) x d (magnitude of displacement) x cos

(W=F x d)

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4
Q

If there is no force, then

A

No work is being done

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5
Q

If the magnitude of the force is 0, then

A

No work is done

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6
Q

Magnitude of the force is

A

Constant over the displacement

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7
Q

1 joule of work is expended when

A

A force of 1 N acts over displacement of 1L

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8
Q

Unit of work is

A

Joule

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8
Q

Work & kinetic energy have units of

A

Joule

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8
Q

Joule is the combination of

A

Newton & Meter

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8
Q

Once joule of work is expended when

A

A force of 1 N acts over a displacement of 1m

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8
Q

Kinetic energy is also called

A

Energy of motion

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9
Q

Kinetic energy is the

A

Energy a mass has by virtue of being in motion

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10
Q

What is the work-energy/work-kinetic energy theorem?

A

The total work done on a system is equal to the system’s change in kinetic energy

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11
Q

Gases that move can

A

Also do work & breathing is a moving gas

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12
Q

State functions are mathematical functions that describe the

A

“State” of a system & can be described as using volume, pressure, or temperature

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13
Q

State functions are

A

Independent of the path by which a system gets to a particular state

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14
Q

An example of a state function is

A

Internal energy, U

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15
Q

What is not a state function?

A

Work

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16
Q

Work depends on

A

The path one takes in getting from the starting point to the end point

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17
Q

Work done by the gas is

A

Path dependent (depends on how you change the state parameters [volume, pressure &/or temp)

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18
Q

What is isochoric?

A

Constant volume

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19
Q

What is isobaric?

A

Constant pressure

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20
Q

The amount of work in a given process is highly dependent on

A

How the pressure & volume change

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21
Q

For changing volume &/or pressure of a gas, the

A

Work is equal to the area under the curve describing the process

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22
Q

The slower the change in volume,

A

The closer the approximation

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23
Q

Energy is defined as

A

The capacity to do work

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24
Q

What is the Law of Energy Conservation?

A

The amount of energy int he universe is constant & is constantly being converted from one form to another

Energy is neither created nor destroyed, but only converted to other kinds of energy

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25
Q

Unit for energy?

A

Joules

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26
Q

One calorie (thermochemical calorie) is

A

Exactly 4.184 J

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27
Q

The food Calorie (capital C) is a

A

Kilocalorie or 1,000cal

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28
Q

The Calorie is an

A

Immense amount of energy

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29
Q

What is potential energy?

A

Energy that is stored bu virtue of position

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30
Q

What is conservative force?

A

Forces that perform no work around a closed path

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31
Q

What can change the potential energy of a system?

A

Only conservative forces

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32
Q

Potential energy can be

A

Recovered & used later

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33
Q

Potential energy is sometimes called

A

Stored energy

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34
Q

What examples of potential energy?

A

Airplane in the air

Battery

Chemical energy in food (sugar, fat)

Thermal energy

Light

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35
Q

Potential energy is the property of a

A

System & not of an isolated object

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36
Q

All energy quantities are

A

Scalar

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37
Q

What is the internal energy?

A

The sum of all the kinetic & potential energies of a system

Results from the state of the particles at a molecular level

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38
Q

What is thermodynamics?

A

The study of energy

How energy is interconverted from one form to another

How energy flows into & out of thermodynamic systems

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39
Q

Everything near a system is called

A

Surroundings

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40
Q

What is the Zeroth Law of thermodynamics?

A
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41
Q

What is the First Law of Thermodynamics?

A

The change in the internal energy of a system is equal to the sum of the heat processed that cause energy to flow into/out of the system & the work done by/on the system

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42
Q

Q>0–>

A

Endothermic process: energy flows into the system

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43
Q

Q<0–>

A

Exothermic process:energy flows out of the system

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44
Q

W<0–>

A

Work done by the system on the surroundings-expansion

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45
Q

W>0–>

A

Work done on the system by the surroundings-Compression

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46
Q

The Second law is sometimes called

A

Entropy Law

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47
Q

Entropy is a measure of

A

Randomness or disorder in a system

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48
Q

Systems that have more randomized, chaotic or evenly mixed have

A

More entrpy

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49
Q

The Second Law states

A

Entropy of the universe is constantly increasing

The universe NEVER & a system almost never spontaneously become more organized

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50
Q

It is not possible to lower a temperature

A

To absolute zero

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51
Q

Heat is energy that is transferred as a result of

A

A temperature difference
(energy flow/process)

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52
Q

Temperature of an ideal gas is

A

Proportional to the average kinetic energy of the particles in a sample of the gas

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53
Q

For a given sample of a single type of gas molecule

A

Not all of the molecules will have the same speed or kinetic energy

(will exhibit a distribution of speeds & kinetic energies)

54
Q

Distribution is

A

Temperature dependent & is called the Maxwell speed distribution

55
Q

The internal energy of an ideal gas is directly

A

Related to the random, disordered motion of the gaseous molecules or atoms

56
Q

What is integer?

A

Find the area under the curve

57
Q

The temperature of the sample depends on the

A

Average kinetic energy

58
Q

Heat capacity is defined as the

A

Ratio between the amount of heat added to or taken away from an object & the change in temperature of the object

59
Q

Unit of heat capacity

A

J/K

60
Q

Heat capacity is an extensive property of

A

Matter

61
Q

Larger samples have greater

A

Heat capacities

62
Q

The heat capacity of a given object depends not only on the mass of that object, but also on the

A

Type of material contained in the object

(specific heat, c)

63
Q

Specific heat & heat capacity are almost always

A

Positive quantities

64
Q

Whenever a quantity is divided by a mass, the term

A

Specific is placed in front of the name of the quantity

65
Q

Water has a large

A

Specific heat; much energy will flow into water

66
Q

Materials with large specific heat are good

A

Thermal insulators

67
Q

Good thermal conductors have low

A

Specific heats

68
Q

What is power

A

The rate of doing work or the rate of expending energy

69
Q

Unit for power

A

watt (W), which is defined as joules/second

(capital W)

70
Q

Gas solubility in liquids is inversely related to

A

Temperature

71
Q

As temperature increases, less

A

Gas is able to dissolve into a liquid

72
Q

An increase in temperature represents

A

Greater kinetic energy

73
Q

Greater kinetic energy allows

A

Dissolved gas molecules to escape & prevents further dissolving

74
Q

Lower temperature slows the kinetic energy of gas molecules, allowing

A

Them to dissolve into liquids

75
Q
A
76
Q

The hypothermic patient

A

Retains anesthetic gases in the blood because of increased solubility related to temperature

77
Q

Gas solubility in a liquid is directly proportional to

A

Pressure & is described by Henry’s law

78
Q

The entropy of an isolated system not in equilibrium will

A

Increase over time, approaching a maximum value at equilibrium

79
Q

Energy can be expressed as

A

Mechanical work

Chemical Reactions

Heat

80
Q

Entropy is the universal trend towards

A

Equilibration

81
Q

Entropy is unidirectional & is the movement of energy from a

A

Higher concentration to a lower

82
Q

The greater the gradient difference, the greater the

A

Flow

83
Q

When does Entropy end?

A

When all energy is equally distributed

84
Q

Temperature is the measurement of the

A

Thermal state of an object

85
Q

Heat is thermal energy; temperature is the

A

Quantitative measurement

86
Q

Molecules in a solid state are held together by

A

Intermolecular forces & move about slightly & vibrate

87
Q

Molecules in a liquid are held together by

A

Intermolecular forces & may slide or floe by each other

88
Q

Molecules in a gas move linearly & the attractive forces between molecules are

A

Less than their kinetic energy. They move free from on another

89
Q

Molecules have no

A

Volume

90
Q

Gas molecules exert no force unless they

A

Collide

91
Q

Collision of molecules with each other or the walls of the system do not

A

Decrease the energy of the system

92
Q

Molecules of a gas are in

A

Constant & random motion

93
Q

The temperature of a gas depends on its

A

Average kinetic energy. The energy of a gas is entirely kinetic

94
Q

Temperature & volume in Charles Law, when pressure is the constant is

A

Directly proportional

95
Q

Pressure & volume in Boyle’s law, when temperature is a constant is

A

Inversely proportional

96
Q

Pressure & temperature in Gay-Lussac’s law, when volume is the constant, is

A

Directly proportional

97
Q

Compressing a gas quickly will

A

Intensify the kinetic energy

Temperature will quickly rise proportional to the decrease in volume

98
Q

1N equals

A

9.8=1kg

99
Q

Work is the product of

A

Forces & displacement

100
Q

Kinetic Energy equation

A

KE=1/2mv(squared)

101
Q

What is the work energy theorem

A

Change in the quantity of kinetic energy

102
Q

Work equals

A

pressure x change in volume

103
Q

What is a state function

A

A property whose value does not depend on the path taken to reach the value

104
Q

State functions only depend on

A

Current equilibrium

105
Q

What are path functions?

A

Heat
Work

106
Q

The amount of work depends on

A

The pathway

107
Q

What is energy?

A

The capacity to do work or the exertion of force (PE vs KE)

108
Q

What is the Law of conservation Energy?

A

Energy can neither be created nor destroyed; can only be changed from one form to another

109
Q

the calorie is how many Joules?

A

4.184J

110
Q

PE equation

A

PE=mass x gravity x height

111
Q

Potential energy is _______ energy

A

Stored

112
Q

Kinetic energy equation

A

KE=1/2mv (squared)

113
Q

What is internal energy?

A

Movement of molecules within the system (sum of PE & KE)

114
Q

A substance doesn’t contain heat, but

A

Energy

115
Q

Thermodynamics is the study of

A

Energy & how it is converted from one form to another & flows into & out of a system

116
Q

What is Zeroeth Law?

A

2 systems in equilibrium with a 3rd system are in thermal equilibration with each other; If A=B & B=C, then A=C

117
Q

First law of Thermodynamics?

A

Energy neither created nor destroyed; change U=Q-W (change in internal energy=energy supplied to system minus amount of thermodynamic work done by the system)

118
Q

Second law of Thermodynamics

A

Entropy always increases

119
Q

Third law of Thermodynamics

A

Entropy of a system approaches a constant as temperature approaches absolute zero

120
Q

Entropy is

A

Equilibration of energy; universal trend to equilibration; unit directional; movement of energy from high to low

121
Q

Temperature is the measurement of a

A

Thermal state of an object; numerical ranking & quantitative

122
Q

heat is thermal energy & is

A

Energy that is transferred as a result of temperature differences

123
Q

Internal energy of an ideal gas is

A

Directly related to random disordered motion of the gaseous molecule or atoms

124
Q

The greatest change in temperature occurs

A

After the first hour an anesthetic has been given

125
Q

Liquid to gas requires

A

Energy

126
Q

2500J/600calories is requires to

A

Convert 1g of water into vapor

127
Q

What is the latent key of vaporization?

A

The energy needed to transform a given amount of liquid into a gas & is measured in kilo-joules

128
Q

What is boiling?

A

The temperature where bulk of the liquid at a given pressure concerts to a vapor

129
Q

Temperature of a liquid will

A

NOT rise above its boiling point; the additional heat is transformed liquid into a gas

130
Q

The rate of vaporization depends on the

A

Temperature of the vapor pressure of the liquid & the partial pressure of the liquid above the liquid

131
Q

Vapor pressure & boiling points are

A

Inversely related; the lower the boiling point, the higher the vapor pressure

132
Q

What is relative humidity

A

The amount of water vapor in the air compared to the maximum water vapor the air can hold at that temperature

133
Q

What is specific heat

A

The heat required to raise the temperature of a mass of a given substance by giving temperature 1 degree

134
Q

The Kinetic Molecular Theory focuses on

A

Molecular movement & the forces between molecules

135
Q

Ideal gas law does not

A

Take into account the small volume of gas molecules & their intermolecular interactions

136
Q

Power is the

A

Rate of doing work or rate of expended energy; amount of work to be done in a given amount of time

137
Q

Power formula triangle

A

W with P across from T

Chem/Phys EXAM 2 (3 decks)

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