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Thermal physics

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Title: Thermal physics


1
Topic 3
  • Thermal physics

2
What is Temperature?
3
Temperature
TEMPERATURE determines the direction of flow of
thermal energy between two bodies in thermal
contact
This is another way of saying that if an object
is hotter than another, heat energy will flow
from the hotter object to the colder!
Obvious, but important to remember!
4
Temperature
  • Temperature is also a measure of the average
    random kinetic energy of the particles in a
    substance.

Note that they are not all travelling at the same
speed.
5
Temperature
  • The hotter the temperature, the faster the
    average speed of the particles

Note that they are not all travelling at the same
speed.
6
Thermal equilibrium
Two bodies in thermal contact will eventually
reach the same temperature. The two bodies are
now said to be in thermal equilibrium.
WARM
WARM
7
Celcius Scale
  • In the Celcius scale, a value of zero degrees is
    assigned to the freezing point of water, and a
    value of one hundred degrees to the boiling point
    of water.

8
Making a Celcius thermometer
  • Place a glass tube containing mercury in a
    mixture of ice and water and labelling the
    position of the mercury as zero.

0C
9
Making a Celcius thermometer
  • Then place the tube in boiling water and label
    the new length as 100C.

100C
0C
10
Making a Celcius thermometer
  • Finally the range from 0 to 100 is subdivided
    into equal intervals.

11
Pressure and Temperature
  • http//phet.colorado.edu/sims/ideal-gas/gas-proper
    ties_en.jnlp

12
Kelvin Temperature
  • Lord Kelvin
  • 1824-1907

13
Kelvin Temperature
  • Kelvin temperature is proportional to the
    average random kinetic energy of the particles in
    a substance.

Note that they are not all travelling at the same
speed.
14
Absolute/Kelvin temperature and Celsius
  • T (in Kelvin) T (in degrees Celcius) 273
  • Just to mention for now that zero Kelvin is the
    lowest possible temperature.

15
Measuring temperature
  • The thermometer has to be placed in thermal
    contact with whatever is being measured until the
    thermometer and object are in thermal equilibrium.

100C
0C
16
So what is heat?
  • Heat is the amount of thermal energy. For
    example, the sparks from a sparkler are at around
    800C but do not burn your skin. However, a hot
    cup of tea at around 100C will burn your hand
    badly. This is because the tea contains more heat
    energy, even though it is cooler. Thermal energy
    is transferred by a temperature difference.

17
Internal Energy
  • This is the sum of the kinetic energies and
    potential energies of the particles in a substance

If you imagine the forces between particles as a
spring, you can see if the particles are pulled
apart or squashed together that energy is stored
in the spring. Similarly there is potential
energy between the particles in a substance.
18
Internal Energy
  • The internal energy of a substance can be
    changed by heating it (or taking heat from it) or
    by doing work on the object (or having the object
    do work).

19
Moles!
20
Moles!
  • Equal masses of different elements will contain
    different numbers of atoms (as atoms of different
    elements have different masses)

21
Moles!
  • It is sometimes useful for physicists and
    chemists (but we dont care about them) to
    compare the number of atoms or molecules in an
    amount of substance.
  • To do this we use the idea of moles.

A chemist
22
Moles!
You need to learn this definition.
  • One mole of a substance contains the same number
    of molecules/atoms as in 12 grams of carbon-12.
  • This number (of atoms or molecules) is known as
    the Avogadro constant (NA) which is equal to 6.02
    x 1023

23
How big is 6.02 x 1023?
  • Imagine the floor of this classroom covered in
    unpopped popcorn

24
How big is 6.02 x 1023?
  • Imagine the all the floors in the school covered
    in unpopped popcorn

25
How big is 6.02 x 1023?
  • Imagine the whole of Busan covered in unpopped
    popcorn

26
How big is 6.02 x 1023?
  • Imagine the whole of Korea covered in unpopped
    popcorn

27
How big is 6.02 x 1023?
  • Imagine the whole of Europe covered in unpopped
    popcorn

You are here!
28
How big is 6.02 x 1023?
  • Imagine the whole of Europe covered in unpopped
    popcorn to a depth of 6 miles!

You are here!
29
How big is 6.02 x 1023?
  • Imagine the whole of Europe covered in unpopped
    popcorn to a depth of 6 miles! Count the grains
    and that is 6 x 1023!
  • 600000000000000000000000
  • Thats how big 6.02 x 1023 is!

30
Moles!
You need to learn this definition.
  • One mole of a substance contains the same number
    of molecules/atoms as in 12 grams of carbon-12.
  • This number (of atoms or molecules) is known as
    the Avogadro constant (NA) which is equal to 6.02
    x 1023

31
Moles!
  • For example, Hydrogen (H2) has a relative
    molecular mass of 2, so 2 grams of hydrogen (one
    mole) contains the same number of molecules as
    atoms in 12g of carbon-12 (6.02 x 1023)

32
Moles!
  • It follows therefore that 7g of lithium (atomic
    mass 7), 20g neon (atomic mass 20) or 39 g
    potassium (atomic mass 39) all contain the same
    number of atoms (1 mole or 6.02 x 1023 atoms)

33
Moles!
  • The number of moles of a substance can thus be
    found by dividing the mass of substance by its
    relative atomic or molecular mass
  • n mass/RAM

34
Example
  • How many moles of sulphur atoms are there in
    80g of sulphur? How many grams of carbon would
    have the same number of atoms?

35
Example
  • How many moles of sulphur atoms are there in
    80g of sulphur? How many grams of carbon would
    have the same number of atoms?
  • N mass/RAM 80/32 2.5 moles

36
Example
  • How many moles of sulphur atoms are there in
    80g of sulphur? How many grams of carbon would
    have the same number of atoms?
  • N mass/RAM 80/32 2.5 moles
  • Mass of carbon RAM x n 12 x 2.5 30 g

37
Relative formula mass
  • We can use the idea of moles and apply it to
    molecules using relative formula mass.
  • C2H5OH
  • RFM (2 x 12) (6 x 1) (1 x 16) 46
  • 46g of ethanol I mole of ethanol molecules

38
Equal volumes
  • Luckily, equal volumes of gas contain the same
    number of particles (at the same temperature and
    pressure)

39
Equal volumes
  • For example, 1 litre of nitrogen contains the
    same number of molecules as there are atoms in
    one litre of Argon.
  • A litre is 1000 cm3 or 1 dm3

40
Mole of gas
  • One mole of any gas occupies 22.4 dm3 (22.400
    cm3 or 22.4 litres) at standard temperature and
    pressure (25C and 1 atmosphere)
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