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2/20/2015
1
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Defining Temperature
* We associate temperature with how hot or cold
an object feels.
* Our sense of touch serves as a qualitative
indicator of temperature.
* Energy must be either added or removed from
an object to change its temperature.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Temperature is proportional to the kinetic
energy of atoms and molecules.
* Temperature is a measure of the average kinetic
energy of the particles in a substance.
* A substance temperature increases as a direct
result of added energy being distributed among
the particles of a substance.
* Internal energy is the
energy of a substance due
to both the random motions
of its particles and to the
potential energy that results
from the distances and
alignments between the
particles.
2/20/2015
2
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Temperature is proportional to the kinetic
energy of atoms and molecules.
* The internal energy of a material is due to the
random motions of its component particles and is
equal to the total energy of those motions.
* The particles can be atoms or molecules, and
they can have three forms of energy:
translational, rotational, and vibrational. .
* Translational energy → is energy that comes
from the horizontal or vertical motion of particles.
* Rotational Energy → is energy that comes from
the rotation or spinning of the particle.
* Vibrational energy → is energy that comes from
the bending or stretching of the bonds within the
particles.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Kinds of Energy
Visual Concept
2/20/2015
3
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Thermal expansion
* In general, if the temperature of a substance
increases, so does its volume. This phenomenon is
known as thermal expansion.
* Different substances undergo different amounts
of expansion for a given temperature change.
* The thermal expansion characteristics of a
material are indicated by a quantity called the
coefficient of volume expansion.
* Gases have the largest values for this
coefficient. Solids typically have the smallest
values.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Thermal expansion
* In general, when the temperature of a material
increases its volume also increases, regardless of
whether the material is a solid, liquid, or gas.
Visual Concept
2/20/2015
4
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Thermal expansion
* In general, the volume of a liquid tends to
decrease with decrease temperature.
* However, the volume of water increases with
decreasing temperature in the range between 0°C
and 4°C.
* When water freezes, crystal form which have more
empty space between the molecules than the
liquid. This explains why ice floats in liquid water .
* Solids typically have the smallest coefficient of
volume expansion values. For this reason, liquids in a
solid container expand more than the container.
This property allows some liquids to be used to
measure changes in temperature.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Measuring Temperature
* Temperature is measured in one of three
common temperature scales:
* Celsius Degrees
* Fahrenheit Degrees
* Kelvin
* To have a temperature scale we need to
know the values for:
* The freezing point of pure water
* The boiling point of pure water
* The number of units between them.
* DEGREE is a unit between 2 points in a
temperature scale.
2/20/2015
5
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Fahrenheit Scale
* Most commonly used in the USA
* Developed in the early 1700’s by Gabriel
Fahrenheit.
* Pure water freezes at 32°F
* Pure water boils at 212°F
* There are 180 equal units or degrees between
the freezing point and boiling point.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Celsius Scale
* Most commonly used in the rest of the world
* Developed in 1740 by Andre Celsius
* Pure water freezes at 0°C
* Pure water boils at 100°C
* There are 100 equal units or degrees between
the freezing point and boiling point.
2/20/2015
6
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Kelvin
* Most commonly used in the scientific world.
* Pure water freezes at 273 K
* Pure water boils at 373 K
* There are 100 equal units between the
freezing point and boiling point.
* Kelvin scale of temperature does not use the
suffix degrees.
* Kelvin scale is referred to as the absolute
scale.
* The 0 temperature in the Kelvin Scale is
referred to as the absolute zero.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Measuring Temperature
* In order for a device to be used as
a thermometer, it must make use of
a change in some physical property
that corresponds to changes in
temperature, such as the volume of
a gas or liquid, or the pressure of a
gas at a constant volume.
* The most common thermometers
use a glass tube containing a thin
column of mercury, colored alcohol,
or colored mineral spirits.
* When the thermometer is heated,
the volume of the liquid expands.
* The change in length of the liquid
column is proportional to the
temperature.
2/20/2015
7
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Changes in temperature
* Matter exists in one of three states:
* solid * liquid * gas
* Matter can change from one state to another
when there is a change in the kinetic energy or
temperature of the object.
* Melting occurs when a solid becomes a liquid.
* The melting point is the point at which melting
begins.
* Melting begins when the particles of a solid
start vibrating fast enough so that they start
breaking away from one another and become
a liquid.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Changes in temperature
* Freezing occurs when a liquid turns into a solid.
* The freezing point is the point at which freezing begins.
* At the freezing point, a liquid particle loses energy. They
don’t move as quickly and eventually become a solid.
* The melting point and the freezing point of a substance
are the same.
* Above the freezing / melting point, the substance is a
liquid.
* Below the freezing / melting point, the substance is a
solid.
* At the freezing / melting point, the substance can be
either a liquid or a solid. * The freezing / melting point of water is 0°C
Below
0°C Water is neither solid nor liquid
15°C Water is liquid Above
-15°C Water is solid (ice)
2/20/2015
8
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Changes in temperature * Evaporation is the process by which a liquid becomes a
gas.
* Particles in liquids move at different speeds. The fastest
moving particles escape from the surface of a liquid
becoming gas.
* Since warmer liquids have faster moving particles,
evaporation occurs more quickly when a substance is
warmer.
* Boiling is another process that allows a liquid to become a
gas.
* When heated, particles within a liquid from bubbles of gas.
When these bubbles of gas start moving fast enough they
rise to the surface of the liquid and escape.
* The boiling point is the point at which a boiling can occur.
* Evaporation can occur at many temperatures, but boiling
can occur only at or above the boiling point.
* The boiling point of water is 100°C.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Changes in temperature * The boiling point of water is 100°C.
* The boiling point of water changes with altitude, because
there is less pressure at higher altitudes, bubbles in the water
vapor need less energy to escape from a liquid.
3000 meters
Water boils at 89°C
Water boils at 100°C
Less Pressure
More Pressure
Sea Level
2/20/2015
9
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Changes in temperature * Condensation occurs when a gas turns into a liquid. * Condensation, like evaporation occurs at a wide range of temperatures. * Particles in gas move more slowly near a cool surface and may form a liquid at the cooler surface. * Most gases condense when its temperature is reduced below the substances boiling point. * Sublimation occurs when a solid turns directly into a gas without going through a liquid phase. * Dry ice, which is frozen Carbon dioxide (CO2), turns directly into carbon dioxide gas under normal temperature conditions. * Deposition occurs when a gas turns directly into a solid without going through a liquid phase.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Changes in temperature GAS.
LIQUID.
SOLID
.Meltin
g
.Fre
ezin
g
Freezing /
Melting
point
Eva
po
ratio
n
Con
de
nsa
tio
n
Boiling
point
.Su
blim
atio
n
Dep
ositio
n
* Boiling is another way of changing a liquid
into a gas.
2/20/2015
10
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Changes in temperature * The temperature scales most widely used today are the Fahrenheit, Celsius, and Kelvin scales * Celsius and Fahrenheit temperature measurements can be converted to each other using this equation: * TF = 1.8 TC + 32° * Temperature in Fahrenheit = 1.8 * temperature in Celsius + 32° * The number 32.0 indicates the difference between the ice point value in each scale: 0.0ºC and 32.0ºF * TC = (TF – 32°) / 1.8 * Temperature in Celsius = (temperature in Fahrenheit – 32°) / 1.8
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Changes in temperature
* Temperature values in the Celsius and
Fahrenheit scales can have positive, negative,
or zero values
* But because the kinetic energy of the atoms
in a substance must be positive, the absolute
temperature that is proportional to that energy
should be positive also.
* A temperature scale with only positive values
is suggested by the graph on the next slide. This
scale is called the Kelvin scale.
2/20/2015
11
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Changes in temperature
* A temperature difference of one degree is the
same on the Celsius and Kelvin scales. The two
scales differ only in the choice of zero point.
* Thus, the ice point (0°C) equals 273K, and the
steam point (100°C) equals 373K.
* The Celsius temperature can therefore be
converted to the Kelvin temperature by adding
273.
* TK = TC + 273
* Temperature in Kelvin = Temperature in Celsius
+ 273
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Temperature is a measure of the average kinetic energy
of the particles that make up an object.
* Heat is a flow of energy from an object at a higher
temperature to an object at a lower temperature.
* Heat and temperature are not the same thing.
* Heat and Thermal Energy
* Heat is always the transfer of energy from an object at a
higher temperature to an object of lower temperature.
* Example:
* Ice cubes temp. 0°C
* Bowl temp. 22°C
* In time ice will melt
and the water and the
bowl will have the same
temperature.
* Water and bowl temp 15°C
2/20/2015
12
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Heat and Thermal Energy
* The water and the bowl end up with the same
temperature, which is lower than the original
temperature of the bowl, but higher than the
original temperature of the ice.
* The bowl and the water end up with the same
temperature because the particles of the bowl
and the ice collide among them, gaining or
losing energy.
* When the energy flows from one object to
another, the thermal energy of both objects
changes.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Heat and Thermal Energy
* Thermal energy is the total random kinetic
energy of particles in an object.
* Thermal energy isn’t the same as temperature
because the total amount of particles in the
object’s isn’t the same.
* Example:
* Glass of water temp 22°C
* Lake Superior temp 22°C
* More
particles
of water
* More
Thermal
energy
2/20/2015
13
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Measuring HEAT
* The most common units for measuring heat
are:
* Calorie
* Joule
* One calorie is the amount of energy needed
to raise the temperature of 1 gram of water by
1 degree Celsius.
* Joule is the standard scientific unit in which
heat is measured.
* One calorie is equal to 4.18 Joules.
1 calorie = 4.18 Joules
* In Nutrition Calorie is written with a CAPITAL C,
which is actually known as 1 kilocalorie or 1,000
calories.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * SPECIFIC HEAT
* The Specific heat of a substance is the
amount of energy required to raise the
temperature of 1 gram of the substance by 1
degree Celsius.
* Every substance has its own Specific Heat
* The Specific Heat of water is one calorie per gram per ° Celsius, and since one calorie is
equal to 4.18 Joules then we can say that the
Specific heat of water is 4.18 Joules per gram °C.
.
2/20/2015
14
Chapter 9.1 “Temperature
and Thermal Equilibrium” * SPECIFIC HEAT
* A large value of Specific heat means that the
substance must absorb a big amount of energy
for it to increase its temperature; and it also
means that it must release a big amount of
energy to decrease it temperature.
* The high Specific Heat of water is the reason
why it is used as a coolant in car radiators.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * SPECIFIC HEAT and MASS * Thermal energy is the total random kinetic energy an object has, so it depends on the objects mass.
* Cup of water temp 90°C
* Example:
* Bath tub with water temp 40°C
* More mass = more thermal energy
* The water in the cup will cool faster because
it has less mass even though it’s hotter than the water in the tub. It will take longer for the tub water to cool because it has more mass.
2/20/2015
15
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Heat is transfer of energy from an object at a
higher temperature to an object at a lower
temperature.
* Energy moves heat in three ways:
* conduction
* convection
* radiation
* To control energy we must control
conduction, convection, and radiation.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * CONDUCTION
* Conduction is the process by which energy
moves from one object to another when they are
physically touching.
* For conduction to occur:.
1) Objects must be touching
2) Objects must have different temperatures
* Conduction will happen until the objects are:
1) Not touching
2) Have the same temperature.
* Some materials are better then others to transfer
energy (heat).
* Conductors→ are materials that transfer energy
(heat) easily.
2/20/2015
16
Chapter 9.1 “Temperature
and Thermal Equilibrium” * CONDUCTION
* Some materials are better then others to
transfer energy (heat).
* Conductors→ are materials that transfer
energy (heat) easily.
* Conductors have:
* Low values of Specific heat
* Examples: most metals
* Insulators→ are materials that do NOT transfer
energy (heat) easily.
* Insulators have:
* High values of Specific heat
* Examples: wood and plastic.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * CONDUCTION
2/20/2015
17
Chapter 9.1 “Temperature
and Thermal Equilibrium” * CONVECTION * Convection is the process that transfers
energy by the movement of large numbers of
particles in the same direction within liquids and
gases.
* With an increase in energy there is an increase
in kinetic energy, particles spread out (thermal
expansion). When particles spread out they
reduce their density. When the density is
reduced a substance goes up.
Chapter 9.1 “Temperature
and Thermal Equilibrium” * CONVECTION
1) Warmer less dense air is
pushed up by the cooler
denser air.
2) As the air cools, it
becomes more dense
and starts to sink. 3) Sinking air moves under
the warmer air, pushing it
back up so that the cycle
repeats. * Convection in large bodies of water (lakes
and oceans) influence the temperature of
the nearby land.
2/20/2015
18
Chapter 9.1 “Temperature
and Thermal Equilibrium” * CONVECTION
Chapter 9.1 “Temperature
and Thermal Equilibrium” * RADIATION * Radiation is the energy that travels as
electromagnetic waves..
* Radiation includes:
* microwaves
* Infrared light
* Visible light
* The sun is the most significant source of
radiation, but all objects emit radiation and
release energy.
2/20/2015
19
Chapter 9.1 “Temperature
and Thermal Equilibrium” * RADIATION
* Radiation from the sun
* Transfer to objects and
persons
* Objects become warmer.
* Particles move faster.
* Thermal
expansion occurs
Chapter 9.1 “Temperature
and Thermal Equilibrium” * CONDUCTION CONVECTION & RADIATION
* Similarities → transfer energy (heat) from warmer
objects to cooler objects.
* Differences → Radiation travels through empty
space.
2/20/2015
20
Chapter 9.1 “Temperature
and Thermal Equilibrium” * Different materials are used to control the
transfer of energy.
* Energy is always being transferred between
objects that coexist at different temperatures.
* Insulators are used to control the flow of energy
(heat) because they are poor conductors.
* Insulators are the materials that keep cool things
cool and hot things hot.
* An insulators is an energy trapper, it prevents
energy from flowing.
* Good insulators include: * Wood * Plastic
* Fiber glass * air
* Shinny materials that
reflect radiation