1. Chapter 19 Temperature scales: Fahrenheit, Celsius (centigrade), Kelvin Thermal expansion The ideal gas law Part 3 Thermodynamics Chapter 19: Temperature and the Ideal Gas Law Reading assignment: Chapter 20.1-20.5 Homework :(due Wednesday, Nov. 30, 2005): Problems:Chapter 19: 1, 14, 17, 28, 30 Chapter 20: 3, 5, 13, 20, 28, 32

2. Temperature Scales: Reliable and quantifiable way of measuring how “hot” an object is.

3. Fahrenheit (1686-1736) established three fixed points on his thermometer. 0 degrees: temperature of an ice, water, and salt mixture. 32 degrees: water-ice combination stabilized at "the thirty-second degree." 98 degrees: “when the thermometer is held in the mouth or under the armpit of a living man in good health." Celsius (1701-1744) established two fixed points on his thermometer. 0°C: representing the freezing point of water. 100°C: the boiling point of water. Kelvin (1834-1907) used the same gradation as Celsius but set his zero point at absolute zero (All molecular motion ceases at absolute zero).

4. How to convert from one temperature scale to another: Where T C, T F, T is the temperature in Celsius (centigrade), Fahrenheit and Kelvin, respectively Kelvin is the proper SI unit

5. “When the thermometer is held in the mouth or under the armpit of a living man in good health” it indicates 98 F (Can fluctuate between 97.5F and 98.9F). Black board example 19.1 a)What is the temperature in Celsius (centigrade)? b)What is the temperature in Kelvin?

6. Heat is the energy that flows between objects because of their difference in temperatures Heat is thermal energy on the move Technically: object’s don’t contain heat Thermal equilibrium Two objects are in thermal equilibrium when they have the same temperature.  They cease to exchange heat. Zeroth law of thermodynamics: If object A and B are separately in thermal equilibrium with a third object C (thermometer), then objects A and B are in thermal equilibrium.

7. Heat and Temperature Touching objects exchange thermal energy –Microscopically, energy flows both ways –On average, energy flows one way Temperature predicts energy flow direction –Energy flows from hotter to colder –No flow  thermal equilibrium  same temp Temperature turns out to be –average thermal kinetic energy per particle More on heat in Chapter 20

8. Thermal expansion of solids and liquids When objects are heated up they typically expand. This is due to the increased motion of molecules at elevated temperatures. Change in Length:  … coefficient of linear expansion L i … initial length  L … change in length  T …change in temperature (in centigrade or Kelvin)

9. Application: Bimetallic strip

10. The New River Gorge Bridge in West Virginia is a steel arch bridge 518 m in length. (alpha=11 x 10 -6 /C) How much does its length change between temperature extremes of -20.0°C and +35.0°C Black board example 19.2 Problem 19. 8

11. Thermal expansion of solids and liquids When objects are heated up they typically expand. This is due to the increased motion of molecules at elevated temperatures. Change in Volume:  … coefficient of volume expansion V i … initial volume  V … change in volume,  T …change in temperature (in centigrade or Kelvin)

12. The Unusual behavior of water. Or: What is the temperature at the bottom of a deep lake? Or: Why does a lake freeze from the top and not the bottom?

13. The ideal gas law Idealized assumptions (work well for many gases at medium temperatures and low pressures): -Gas molecules don’t interact upon collision -Molecular volume of gas molecules is negligible compared with volume of container P … Pressure of gas V … Volume of gas n … number of moles of gas R … Universal gas constant, R = 8.315 J/mol·K T … absolute Temperature (in Kelvin)!!

14. Nine grams of water are placed in a 2.00 L pressure cooker and heated to 500°C. Black board example 19.3 Problem 19.28 What is the pressure inside the container if no gas escapes?