1. Thermodynamics
Thermodynamics is the study of the transfer of energy, as heat.
Internal energy of a substance is the total kinetic energy of a substance due to the motion of the particles in the substance.

2. Temperature
Temperature measure of the average internal kinetic energy of the particles in a substance. Measure of internal energy within a substance Measure of how much the atoms and molecules of a substance are moving. Temperature changes only when energy is added or removed. This is known as heat.

3. Thermometer Thermometer instrument used to measure temperature.
“Thermos” means heat and “metros” to measure.
The most common thermometers use a glass tube containing a thin column of mercury, or alcohol.
Energy is absorbed, and the volume of the liquid expands up the glass column.

4. Three different types of scales used for measuring temperature.
Temperature Scales
Three different types of scales used for measuring temperature.
Fahrenheit Scale Created by German physicist, Daniel Gabriel Fahrenheit ( ) in Set the freezing point of water at 32° and the boiling point at 212°. With these two points the bases were created 180 degrees apart.
Celsius Scale Proposed by Swedish astronomer, Anders Celsius ( ) in Using the same idea, he determined the freezing temperature for water to be 0° and the boiling temperature 100 °.The Celsius scale is the most used in the world.
Kelvin Scale Proposed by William Thomson, Lord Baron Kelvin. This scale is based on absolute zero with K for the freezing point, and K for the boiling point, of water.

5. Temperature Scales Uses
Temperature is measured in degrees on the Fahrenheit, Celsius, and Kelvin scales.
Temperature scales and their uses
Scale
Ice Point
Steam Point
Applications
Fahrenheit
32°F
212°F
meteorology, medicine, & nonscientific uses (U.S.)
Celsius
0°C
100°C
meteorology, medicine, & nonscientific uses (outside U.S.); other sciences (International)
Kelvin (absolute) K K
physical chemistry, gas laws, astrophysics, thermodynamics, low-temperature physics

6. Absolute Zero
William Thomson, Baron Kelvin. Understood that there was a limit to how cold something can be.
The Kelvin scale goes to a temperature of Absolute Zero-the temperature at which nothing could be colder and no heat energy remains in a substance — there is no motion and no kinetic energy.
Absolute zero is where all molecular motion stops and is the lowest temperature possible.
Absolute Zero occurs at 0 Kelvin or °C at ° Fahrenheit
Absolute zero has never been reached. The closest laboratory experiments have reached is a temperature of K.

9. Temperature Conversions
Celsius to Fahrenheit °F = (°C 9/5) +32
Fahrenheit to Celsius °C = (°F-32) (5/9)
Celsius to Kelvin K = °C
Kelvin to Celsius °C = K
U.S. Weather
Mexico Weather

10. Conversion Examples K = °C + 273.15 K = °19 + 273.15 K = 292.15
°C = (°F-32) (5/9)    
°C = (°78-32).556
°C = 25.57°
°F = (9/5)(°C) +32  
°F = (1.8)(°11)+32
°F= °51.8

12. Heat Heat (Q) is the transfer of energy (given up or absorbed)
between objects because of a difference in their internal energies, or temperatures.
The direction in which energy travels as heat can be explained at the atomic level.
Energy transferred as heat always moves from an object at
higher temperature to an object at lower temperature.

13. Heat Exchange
Heat may be transferred from one substance to another three ways: conduction, convection, and radiation.
When two objects reach equal temperatures, this is known as thermal equilibrium.

14. Conduction
Conduction transfer of heat energy by direct contact
Conduction involves the transfer of energy from one molecule to adjacent molecules without the substance as a whole moving. (Particularly a transfer for solids) 14

15. Convection
Convection is the transfer of heat energy in circular currrents due to change in density, takes place in fluids i.e., liquids and gases 15

16. Radiation
Radiation is the transfer of heat energy in the form of electromagnetic radiation, specifically infrared waves,. 16

17. Specific Heat Capacity
Specific Heat Capacity (C) The quantity of energy needed to raise the temperature of 1kg of a substance by 1˚C at constant pressure.
Since different substances have different compositions, different substances have different heat capacities.
Specific Heat Capacity = energy transferred as heat
mass × change in temperature
C = Q/(mΔT)
units: J/(kg˚C) 17

18. Specific Heat Capacities
The high specific heat of water plays an important role in temperature regulation.
Substance
Cp (J/kg˚C)
water
4.186x103
Ice
2.09x103
steam
2.01x103
aluminum
8.99x102
glass
8.37x102
iron
4.48x102
copper
3.87x102
silver
2.34x102
gold
1.29x102
lead
1.28x102
mercury
1.38x102 18

19. Heat Heat (Q) is the measure of the exchange of energy.
It is dependent on the mass of the substance, the specific heat capacity, and the change in temperature
Q = mCDT
units: kg (J/(kg˚C) ˚C = JOULES
Calorie (cal) is the quantity of heat required to raise the temperature of one gram of water one degree Celsius Joules = 1 cal
British thermal unit (Btu) English unit commonly used in the United States

20. Thermal Units Joule (J) Equal to 1 kg (m2/s2) Calorie (cal) 4.186 J
Heat Unit
Equivalent value
Uses
Joule (J)
Equal to 1 kg (m2/s2)
SI unit of energy
Calorie (cal)
4.186 J
Non-SI unit of heat; found especially in older works of physics and chemistry
Kilocalorie (kcal)
4.186x103 J
Non-SI unit of heat
Calorie, or dietary Calorie
4.186x103 J = 1 kcal
Food and nutritional science
British thermal unit (Btu)
1.055x103 J
English unit of heat; used in engineering, air-conditioning, and refrigeration
Therm
1.055x108 J
Equal to Btu; used to measure natural-gas usage

22. Thermal Equilibrium
Thermal equilibrium is the basis of measuring temperature with thermometers
Ex: Can of warm fruit juice immersed in a large beaker of cold water
After 15 minutes, the can will be cooler and the water will be slightly warmer
Eventually they will be at the same temperature. This is an example of thermal equilibrium.
Energy transferred as Heat travels from objects of higher temperature to objects of lower temperature.

23. Thermal Expansion
Thermal Expansion the tendency of matter to change in volume in response to a change in temperature.
Thermometers are an example of thermal expansion- most contain a liquid which is constrained to flow in only one direction (along the tube) due to changes in volume brought about by changes in temperature. 23