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Heat and Thermodynamics: Understanding Temperature, Heat, and Energy Transformation

This text explores the concepts of temperature and heat, the difference between them, and their applications in various systems. It also discusses the need for efficient energy usage and the development of new energy sources. The text explains the laws of thermodynamics and how temperature is measured using different scales. It concludes with a mention of absolute zero and the Kelvin scale.

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Heat and Thermodynamics: Understanding Temperature, Heat, and Energy Transformation

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  1. L 16 Heat and Thermodynamics [1] • What is temperature? • How is it measured? • What is heat? • What is the difference between heat and temperature? • Applications: engines, refrigerators, air conditioners, human body, electric power production systems • It’s all about how ENERGY is used.

  2. The US uses about 25 % of the total World and US energy Consumption Organization for Economic Co-operation and Development

  3. Energy use by source • Existing energy source must be used more efficiently, and • New energy sources must be developed

  4. Hot toast Temperature is not the whole story! • Cake and pan just taken out of a 400° oven. • Both are at 400° • You can touch the cake, but not the pan! • You can handle toast right out of the toaster • You can eat the pie crust, but not the filling.

  5. Drilling or grinding • After drilling into a piece of metal, the drill bit is very hot • The metal being grinded also gets hot • You can also get the bit or the metal hot by placing it in a torch • Is there a difference in the outcome?

  6. “Engines” • Any device which uses heat to do work • Steam engine, internal combustion engine Burn fuel  boil water (steam)  push piston (work) steam Hero’s engine steam HEAT

  7. Human engine • The human body is an engine. • Food in  metabolism  work out • Energy in   Energy out • We are all subject to the laws of thermodynamics BODY ENGINE

  8. Internal energy & temperature • All systems have internal energy • The internal energy is the sum of the energy of all the molecules in the system • For example- in a gas the molecules are in random motion, each molecule has kinetic energy = ½ m v2 • If we add up all the kinetic energies of all the molecules we get the internal energy

  9. System C System B System A Energy transfers All systems (living organisms and mechanical) are continually exchanging energy with other systems or their environment.

  10. Energy transfer examples • Ice melts in water • water boils • steam condenses to water • Water  ice in freezer • Pop cools in refrigerator • The sun warms you on an autumn day • Antifreeze is circulated through your car engine to maintain a steady temperature

  11. Thermodynamics • Is the study of heat energy and its transformation into mechanical energy. • Is a set of a few basic empirical(based on observations) rules that place limits of how these transformations can occur, and how efficiently they can be carried out.

  12. Engine Work out energy in Work out Efficiency = Energy in Engines If we convert all of the energy taken in to work the efficiency would be 100%

  13. Laws of thermodynamics in a nutshell • You can’t get more work out than the energy you put in (conservation of energy). • You can’t even get as much out as you put in (engine efficiency cannot be 100%) heat energy cannot be converted completely to useful energy (work)

  14. Internal combustion engine 100% 62 % 16% 10% 8.8% 3.2%

  15. How is temperature measured? • We use the fact that the properties of materials change with temperature • For example: • Metals expand with increasing temp • Length of liquid column expands • Electrical resistance changes • Pressure of a gas increases with temperature • Infrared emission from objects changes color

  16. Can we trust our senses of hot and cold? Will both fingers feel the same temperature when they are put in the warm water?

  17. Length of a mercury column • The length of the Hg column increases with temperature • How is the thermometer calibrated? •  temperature scales • Fahrenheit • Celsius • Kelvin Mercury column Mercury reservoir

  18. Temperature scales: based on freezing and boiling points of water Celsius scale Fahrenheit scale boiling point 212° 100° 100° 180° freezing point 32° 0°

  19. Centigrade & Fahrenheit scales • Scales are offset ( 0 °F is not 0°C) • Celsius scale is compressed compared to the Fahrenheit scale • 1°C = 180/100 = 9/5 °F • Conversion formulas: • TC = (5/9)  (TF – 32) • TF = (9/5  TC) + 32

  20. Examples 1) What is the temperature in C if the temperature is 68°F? TC = (5/9) (TF – 32 ) = (5/9)(68 – 32) = (5/9)  (36) = 20°C 2) What is the temperature in F if the temperature is – 10 °C? TF = (9/5  TC) + 32 = (9/5  – 10) + 32 = – 18 + 32 = 14°F

  21. Absolute zero – as cold as it gets! • There is nothing particularly significant about 0°C or 0°F. • Is there a temperature scale where 0 really is ZERO? It doesn’t get any colder than this! • YES– It is called the KELVIN scale. • At zero Kelvin, all molecular motion stops. • We can see this from the behavior of gases,where pressure decreases with temperature.

  22. Gas Pressure °C 273.15 °C Approaching absolute zero As a gas is cooled, its pressure decreases. If we imagine continuing to cool it, the P vs T plot for all quantities of gas extrapolate to - 273.15 C This is absolute zero!

  23. Kelvin scale (where 0 means 0) • TK = TC + 273.15° • One degree K = one degree C • There are NO negative Kelvin temperatures, zero is the minimum.

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