Chapter 16

Temperature

and the

Kinetic Theory of Gases

Overview of Thermodynamics Extends the ideas of temperature and internal

energy Concerned with concepts of energy transfers

between a system and its environment And the resulting variations in temperature or

changes in state Explains the bulk properties of matter and the

correlation between them and the mechanics of atoms and molecules

Temperature We associate the concept of temperature with

how hot or cold an objects feels Our senses provide us with a qualitative

indication of temperature Our senses are unreliable for this purpose We need a reliable and reproducible way for

establishing the relative hotness or coldness of objects that is related solely to the temperature of the object Thermometers are used for these measurements

Thermal Contact Two objects are in thermal contact

with each other if energy can be exchanged between them The exchanges can be in the form of heat

or electromagnetic radiation The energy is exchanged due to a

temperature difference

Thermal Equilibrium Thermal equilibrium is a situation in

which two object would not exchange energy by heat or electromagnetic radiation if they were placed in thermal contact The thermal contact does not have to also

be physical contact

Zeroth Law of Thermodynamics If objects A and B are separately in

thermal equilibrium with a third object C, then A and B are in thermal equilibrium with each other Let object C be the thermometer Since they are in thermal equilibrium with

each other, there is no energy exchanged among them

Zeroth Law of Thermodynamics, Example

Object C (thermometer) is placed in contact with A until it they achieve thermal equilibrium

The reading on C is recorded Object C is then placed in contact with object B until they

achieve thermal equilibrium The reading on C is recorded again

If the two readings are the same, A and B are also in thermal equilibrium

Temperature Temperature can be thought of as the

property that determines whether an object is in thermal equilibrium with other objects

Two objects in thermal equilibrium with each other are at the same temperature If two objects have different temperatures, they

are not in thermal equilibrium with each other

Thermometers A thermometer is a device that is used

to measure the temperature of a system Thermometers are based on the

principle that some physical property of a system changes as the system’s temperature changes

Thermometers, cont The properties include

The volume of a liquid The length of a solid The pressure of a gas at a constant volume The volume of a gas at a constant pressure The electric resistance of a conductor The color of an object

A temperature scale can be established on the basis of any of these physical properties

Thermometer, Liquid in Glass A common type

of thermometer is a liquid-in-glass

The material in the capillary tube expands as it is heated

The liquid is usually mercury or alcohol

Calibrating a Thermometer A thermometer can be calibrated by

placing it in contact with some environments that remain at constant temperature

Common systems involve water A mixture of ice and water at atmospheric

pressure Called the ice point or freezing point of water

A mixture of water and steam in equilibrium Called the steam point or boiling point of water

Celsius Scale The ice point of water is defined to be

0oC The steam point of water is defined to

be 100oC The length of the column between these

two points is divided into 100 equal segments, called degrees

Problems with Liquid-in-Glass Thermometers An alcohol thermometer and a mercury

thermometer may agree only at the calibration points

The discrepancies between thermometers are especially large when the temperatures being measured are far from the calibration points

Gas Thermometer The gas thermometer offers a way to

define temperature Also directly relates temperature to internal

energy Temperature readings are nearly

independent of the substance used in the thermometer

Constant Volume Gas Thermometer

The physical change exploited is the variation of pressure of a fixed volume gas as its temperature changes

The volume of the gas is kept constant by raising or lowering the reservoir B to keep the mercury level at A constant

Constant Volume Gas Thermometer, cont The thermometer is calibrated by using

a ice water bath and a steam water bath The pressures of the mercury under

each situation are recorded The volume is kept constant by adjusting A

The information is plotted

Constant Volume Gas Thermometer, final To find the

temperature of a substance, the gas flask is placed in thermal contact with the substance

The pressure is found on the graph

The temperature is read from the graph

Absolute Zero The thermometer

readings are virtually independent of the gas used

If the lines for various gases are extended, the pressure is always zero when the temperature is –273.15o C

This temperature is called absolute zero

Absolute Temperature Scale Absolute zero is used as the basis of

the absolute temperature scale The size of the degree on the absolute

scale is the same as the size of the degree on the Celsius scale

To convert: TC = T – 273.15 TC is the temperature in Celsius T is the Kelvin (absolute) temperature

The absolute temperature scale is now based on two new fixed points Adopted in 1954 by the International

Committee on Weights and Measures One point is absolute zero The other point is the triple point of water

This is the combination of temperature and pressure where ice, water, and steam can all coexist

Absolute Temperature Scale, 2

Absolute Temperature Scale, 3 The triple point of water occurs at 0.01o

C and 4.58 mm of mercury This temperature was set to be 273.16

on the absolute temperature scale This made the old absolute scale agree

closely with the new one The unit of the absolute scale is the kelvin

Absolute Temperature Scale, 4 The absolute scale is also called the

Kelvin scale Named for William Thomson, Lord Kelvin

The triple point temperature is 273.16 K No degree symbol is used with kelvins

The kelvin is defined as 1/273.16 of the temperature of the triple point of water

Some Examples of Absolute Temperatures

This figure gives some absolute temperatures at which various physical processes occur

The scale is logarithmic The temperature of

absolute cannot be achieved

Experiments have come close

Energy at Absolute Zero According to classical physics, the kinetic

energy of the gas molecules would become zero at absolute zero

The molecular motion would cease Therefore, the molecules would settle out on the

bottom of the container Quantum theory modifies this and shows

some residual energy would remain This energy is called the zero-point energy

Fahrenheit Scale A common scale in everyday use in

the US Named for Daniel Fahrenheit Temperature of the ice point is 32oF Temperature of the steam point is 212oF There are 180 divisions (degrees)

between the two reference points

Comparison of Scales Celsius and Kelvin have the same size

degrees, but different starting pointsTC = T – 273.15

Celsius and Fahrenheit have difference sized degrees and different starting points

932

5F CT T F

Comparison of Scales, cont To compare changes in temperature

Ice point temperatures 0oC = 273.15 K = 32oF

steam point temperatures 100oC = 373.15 K = 212oF

5

9C FT T T

Thermal Expansion Thermal expansion is the increase in the

size of an object with an increase in its temperature

Thermal expansion is a consequence of the change in the average separation between the atoms in an object

If the expansion is small relative to the original dimensions of the object, the change in any dimension is, to a good approximation, proportional to the first power of the change in temperature

Thermal Expansion, example As the washer is heated, all

the dimensions will increase A cavity in a piece of

material expands in the same way as if the cavity were filled with the material

The expansion is exaggerated in this figure

Linear Expansion Assume an object has an initial length L That length increases by L as the

temperature changes by T The change in length can be found by

L = Li T is the average coefficient of linear

expansion

Linear Expansion, cont This equation can also be written in

terms of the initial and final conditions of the object: Lf – Li = Li(Tf – Ti)

The coefficient of linear expansion has units of (oC)-1

Linear Expansion, final Some materials expand along one

dimension, but contract along another as the temperature increases

Since the linear dimensions change, it follows that the surface area and volume also change with a change in temperature

Thermal Expansion

Volume Expansion The change in volume is proportional to the

original volume and to the change in temperature

V = Vi T is the average coefficient of volume

expansion For a solid, 3

This assumes the material is isotropic, the same in all directions

For a liquid or gas, is given in the table

Area Expansion The change in area is proportional to

the original area and to the change in temperature

A = Ai T is the average coefficient of area

expansion = 2

Thermal Expansion, Example In many situations,

joints are used to allow room for thermal expansion

The long, vertical joint is filled with a soft material that allows the wall to expand and contract as the temperature of the bricks changes

Bimetallic Strip Each substance has

its own characteristic average coefficient of expansion

This can be made use of in the device shown, called a bimetallic strip

It can be used in a thermostat

Water’s Unusual Behavior As the temperature

increases from 0o C to 4o C, water contracts

Its density increases Above 4o C, water

expands with increasing temperature

Its density decreases The maximum density

of water (1 000 kg/m3) occurs at 4oC

Gas: Equation of State It is useful to know how the volume, pressure

and temperature of the gas of mass m are related

The equation that interrelates these quantities is called the equation of state These are generally quite complicated If the gas is maintained at a low pressure, the

equation of state becomes much easier This type of a low density gas is commonly

referred to as an ideal gas

Ideal Gas – Details A collection of atoms or molecules that

Move randomly Exert no long-range forces on one another Are so small that they occupy a negligible

fraction of the volume of their container

The Mole The amount of gas in a given volume is

conveniently expressed in terms of the number of moles

One mole of any substance is that amount of the substance that contains Avogadro’s number of molecules Avogadro’s number, NA = 6.022 x 1023

Moles, cont The number of moles can be

determined from the mass of the substance: n = m / M M is the molar mass of the substance

Commonly expressed in g/mole m is the mass of the sample n is the number of moles

Gas Laws When a gas is kept at a constant

temperature, its pressure is inversely proportional to its volume (Boyle’s Law)

When a gas is kept at a constant pressure, the volume is directly proportional to the temperature (Charles’ Laws)

When the volume of the gas is kept constant, the pressure is directly proportional to the temperature (Guy-Lussac’s Law)

Ideal Gas Law The equation of state for an ideal gas

combines and summarizes the other gas lawsPV = n R T

This is known as the ideal gas law R is a constant, called the Universal Gas

Constant R = 8.314 J/ mol K = 0.08214 L atm/mol K

From this, you can determine that 1 mole of any gas at atmospheric pressure and at 0o C is 22.4 L

Ideal Gas Law, cont The ideal gas law is often expressed in

terms of the total number of molecules, N, present in the sample

P V = n R T = (N / NA) R T = N kB T kB is Boltzmann’s constant

kB = 1.38 x 10-23 J / K

Ludwid Boltzmann 1844 – 1906 Contributions to

Kinetic theory of gases Electromagnetism Thermodynamics

Work in kinetic theory led to the branch of physics called statistical mechanics

Kinetic Theory of Gases Uses a structural model based on the

ideal gas model Combines the structural model and its

predictions Pressure and temperature of an ideal

gas are interpreted in terms of microscopic variables

Structural Model Assumptions The number of molecules in the gas is

large, and the average separation between them is large compared with their dimensions The molecules occupy a negligible volume

within the container This is consistent with the macroscopic

model where we assumed the molecules were point-like

Structural Model Assumptions, 2 The molecules obey Newton’s laws of

motion, but as a whole their motion is isotropic Any molecule can move in any direction

with any speed Meaning of isotropic

Structural Model Assumptions, 3 The molecules interact only by short-range

forces during elastic collisions This is consistent with the ideal gas model, in

which the molecules exert no long-range forces on each other

The molecules make elastic collisions with the walls

The gas under consideration is a pure substance All molecules are identical

Ideal Gas Notes An ideal gas is often pictured as

consisting of single atoms However, the behavior of molecular

gases approximate that of ideal gases quite well Molecular rotations and vibrations have no

effect, on average, on the motions considered

Pressure and Kinetic Energy Assume a container

is a cube Edges are length d

Look at the motion of the molecule in terms of its velocity components

Look at its momentum and the average force

Pressure and Kinetic Energy, 2 Assume perfectly

elastic collisions with the walls of the container

The relationship between the pressure and the molecular kinetic energy comes from momentum and Newton’s Laws

Pressure and Kinetic Energy, 3 The relationship is

This tells us that pressure is proportional to the number of molecules per unit volume (N/V) and to the average translational kinetic energy of the molecules

___22 1

3 2

NP mv

V

Pressure and Kinetic Energy, final This equation also relates the macroscopic

quantity of pressure with a microscopic quantity of the average value of the molecular translational kinetic energy

One way to increase the pressure is to increase the number of molecules per unit volume

The pressure can also be increased by increasing the speed (kinetic energy) of the molecules

A Molecular Interpretation of Temperature We can take the pressure as it relates to the

kinetic energy and compare it to the pressure from the equation of state for an idea gas

Therefore, the temperature is a direct measure of the average translational molecular kinetic energy

___22 1

3 2 B

NP mv Nk T

V

A Microscopic Description of Temperature, cont Simplifying the equation relating

temperature and kinetic energy gives

This can be applied to each direction,

with similar expressions for vy and vz

___

21 3

2 2 Bmv k T

___

21 1

2 2x Bmv k T

A Microscopic Description of Temperature, final Each translational degree of freedom

contributes an equal amount to the energy of the gas In general, a degree of freedom refers to

an independent means by which a molecule can possess energy

A generalization of this result is called the theorem of equipartition of energy

Theorem of Equipartition of Energy The theorem states that the energy of a

system in thermal equilibrium is equally divided among all degrees of freedom

Each degree of freedom contributes ½ kBT per molecule to the energy of the system

Total Kinetic Energy The total translational kinetic energy is just N

times the kinetic energy of each molecule

This tells us that the total translational kinetic energy of a system of molecules is proportional to the absolute temperature of the system

___21 3 3

2 2 2total BE N mv Nk T nRT

Monatomic Gas For a monatomic gas, translational kinetic

energy is the only type of energy the particles of the gas can have

Therefore, the total energy is the internal energy:

For polyatomic molecules, additional forms of energy storage are available, but the proportionality between Eint and T remains

int

3

2E nRT

Root Mean Square Speed The root mean square (rms) speed is

the square root of the average of the squares of the speeds Square, average, take the square root

Solving for vrms we find

M is the molar mass in kg/mole

___

2 3 3Brms

k T RTv v

m M

Some Example vrms Values

At a given temperature, lighter molecules move faster, on the average, than heavier molecules

Distribution of Molecular Speeds The observed speed

distribution of gas molecules in thermal equilibrium is shown

NV is called the Maxwell-Boltzmann distribution function

Distribution Function The fundamental expression that describes

the distribution of speeds in N gas molecules is

mo is the mass of a gas molecule, kB is Boltzmann’s constant and T is the absolute temperature

23

2224

2B

mvk To

VB

mN N v e

k T

Average and Most Probable Speeds

The average speed is somewhat lower than the rms speed

The most probable speed, vmp is the speed at which the distribution curve reaches a peak

2

1.41B Bmp

o o

k T k Tv

m m

81.60B B

o o

k T k Tv

m m

Speed Distribution The peak shifts to the right

as T increases This shows that the average

speed increases with increasing temperature

The width of the curve increases with temperature

The asymmetric shape occurs because the lowest possible speed is 0 and the upper classical limit is infinity

Speed Distribution, final The distribution of molecular speeds

depends both on the mass and on temperature

The speed distribution for liquids is similar to that of gasses

rms mpv v v

Evaporation Some molecules in the liquid are more energetic

than others Some of the faster moving molecules penetrate

the surface and leave the liquid This occurs even before the boiling point is reached

The molecules that escape are those that have enough energy to overcome the attractive forces of the molecules in the liquid phase

The molecules left behind have lower kinetic energies

Therefore, evaporation is a cooling process

Atmosphere For such a huge volume of gas as the

atmosphere, the assumption of a uniform temperature throughout the gas is not valid

There are variations in temperature Over the surface of the Earth At different heights in the atmosphere

Temperature and Height At each location, there is a

decrease in temperature with an increase in height

As the height increases, the pressure decreases

The air parcel does work on its surroundings and its energy decreases

The decrease in energy is manifested as a decrease in temperature

Lapse Rate The atmospheric lapse rate is the

decrease in temperature with height The lapse rate is similar at various

locations across the surface of the earth The average global lapse rate is about –

6.5o C / km This is for the area of the atmosphere

called the troposphere

Layers of the Atmosphere Troposphere

The lower part of the atmosphere Where weather occurs and airplanes fly

Tropopause The imaginary boundary between the troposphere

and the next layer Stratosphere

Layer above the tropopause Temperature remains relatively constant with

height