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Thermal properties of matter
1.
Thermal Properties of Matter
Physics 2
2.
Topic Outline •
Temperature • Thermal expansion • Boyle’s Law • Charles’s Law • Atoms and Molecules • Kinetic Theory of Gases
3.
Temperature A temperature of a body of matter is a measure of the average kinetic energy of random translational motion of its constituent particles. It measures the hotness or coldness of a body.
4.
Thermometer Thermometer is a device used to measure temperature. In Celsius scale the freezing point of water is 0oC and its boiling point is 100oC, and in the Fahrenheit scale, these points are assigned the values of 32oF and 212oF, respectively.
5.
Thermal Expansion Thermal expansion is the change in length in a solid because of the change in temperature.
6.
Coefficients of Linear Expansions
7.
Example:
8.
Volume Expansion
9.
Water Above 4oC water expands when heated. From 0oC to 4oC, however, the volume of a water sample decreases with
ice increasing temperature. Thus water has its maximum density at 4oC.
10.
Boyle’s Law Discovered by Robert Boyle (1627‐1691), states that at constant temperature, the volume of a gas is inversely proportional to its absolute pressure.
11.
Example:
12.
Absolute Temperature Scale The absolute temperature scale has its zero point at ‐273oC; temperature un this scale are measured in Kelvin (K). The Rankine absolute temperature scale has its zero point at ‐ 460oF; temperature in this scale are designated oR. Absolute zero is 0K = 0oR = ‐273oC = ‐460oF.
13.
Charles’s Law Discovered by Jacques Chares, states that at constant pressure, the volume of a gas is directly proportional to its absolute temperature.
14.
Example:
15.
Ideal Gas Law
16.
Atoms and Molecules Elements are the simplest substances of which matter in bulk is composed. The ultimate particles of an elements are its atoms. Two or more elements may combine chemically to form a compound, a substance whose properties are different from those of the elements that compose it. The ultimate particles of a compound in gaseous form are molecules, which consist of the atoms of its constituent elements joined together in a definite way. 1 atomic mass unit = 1 u = 1.66 x 10‐27 kg
17.
Example:
18.
Kinetic Theory of Gases According to the kinetic theory of gases, a gas consists of a great many tiny individual molecules that do not interact with one another except in collisions. The molecules are supposed to be far apart compared with their dimensions and to be in constant motion.
19.
Kinetic Energy and Absolute
Temperature of gases The significance of absolute zero in the kinetic theory of gases is straight forward: It is the temperature at which all molecular translational movement stops.
20.
Molecular Speeds Finding the average speed of gas molecules whose mass is m.
21.
REFERENCE: Modern Technical Physics 6th Edition by
Arthur Beiser Copyright © 1992 by Addison‐Wesley Publishing Company, Inc.