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Energy in Atmosphere

Energy in Atmosphere. Part 1. Atmosphere Formation. Ancient volcanic eruptions released gases into atmosphere Ammonia, Nitrogen , CO 2 , CO, Sulfur, Methane, Hydrogen Water was formed ( meteorites released water when collide w/ Earth ) Algae formed in oceans

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Energy in Atmosphere

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  1. Energy in Atmosphere

  2. Part 1. Atmosphere Formation • Ancient volcanic eruptions released gases into atmosphere • Ammonia, Nitrogen, CO2, CO, Sulfur, Methane, Hydrogen • Water was formed (meteorites released water when collide w/ Earth) • Algae formed in oceans • Photosynthesis uses CO2 to make O2 • O2 diffuses into atmosphere • Ozone layer is formed (O3)

  3. Part 2: Air Pressure • Force exerted by the weight of air • Measured with a barometer • Air Pressure at sea level: • 1 atmosphere • 15 lbs per sq. inch • 30 inches of mercury • 760 mm of mercury • 1013 millibars (mb)

  4. Altitude Temperature Air Pressure Air Pressure Altitude Temperature Part 2: Air Pressure • As altitude increases, air pressure decreases • As temperature increases, air pressure decreases

  5. Part 3: Composition of Atm • Nitrogen = 78% • Oxygen = 21% • Argon = .4% • Greenhouse Gases – absorb Infrared (warming) radiation • CO2 • Water Vapor • Chlorofluorocarbons (CFCs) • Methane • Ozone – filters out UV (skin cancer) radiation

  6. Part 4: Energy • Energy is transferred from warmer to cooler substances • Heat Source = warmer • Heat Sink = cooler • Temperature • Average Kinetic Energy of the particles in a substance • Higher Temp = faster moving particles

  7. Part 5: Heat Transfer Methods • Conduction • Contact between hot substance and cooler substance (touching) • Curling Iron • Convection • Heated material rises b/c it has a lowerdensity • Happens in liquids and gases

  8. Water loses heat to air becoming cooler and more dense Heated water rises Cooler water sinks Water is heated, becomes less dense Convection Cell – one cycle Convection Current – 2 or more cycles

  9. Part 5: Heat Transfer Methods • Radiation • Energy transfer by waves of energy • Sun’s energy to Earth • Example • Light Bulb • Microwave

  10. CREST TROUGH WAVELENGTH Part 6: Electromagnetic Radiation • Vibrating particles have electrical charges that also vibrate forming electromagnetic waves

  11. Frequency Wavelength Part 6: Electromagnetic Radiation • Frequency • Number of crests passing a point in one second • Hertz (Hz) is unit for frequency • As wavelength gets longer, freq gets smaller

  12. Electromagnetic Radiation

  13. Part 7: Electromagnetic Spectrum • Each form of energy has a specific frequency and wavelength • ALL forms travel at speed of light: 186,000 miles/sec or 3x108 m/s • Visible Light – maximum intensity • When waves are absorbed and then re-radiated (given off), they have longer wavelengths

  14. Part 8. Heating of Land and Water • Land absorbs heat energy FASTER and cools FASTER than water • Reasons for Results • Land is darker and rougher, so it is a better absorber and radiator of energy • Water has a higher specific heat so it heats and cools more slowly

  15. Heating of Land and Water • Effects on Earth due to different heating rates of land and water • Climate • Cooler summers near water • Warmer winters near water • Water causes areas near water to have small seasonal changes and temperature ranges

  16. Heating of Land and Water • Air above surface • Air is mainly heated by energy re-radiated from surface (terrestrial radiation) = infrared radiation = longer wavelengths • Since land gives off energy faster, air over land heats and cools faster than air over water

  17. Part 9. World-Wide Air Circulation • Coriolis Effect • Apparent bending of wind b/c of the rotation of the Earth • Northern Hemisphere – wind curves to RIGHT • Southern Hemisphere – wind curves to LEFT • Coriolis effect influences wind direction.

  18. Part 10. Insolation • Greenhouse Effect • Process to heat the atmosphere • Earth absorbsradiation from Sun • Energy is re-radiated to the atmosphere with a longer wavelength (infrared) • Infrared radiation gets absorbed by gases (CO2 and water vapor) and remains trapped in atmosphere

  19. Part 11. Insolation – Temperature Lag • Sun’s energy is first absorbed by Earth’s surface, then given off as infrared radiation which warms the air • There is a time difference (lag time) between greatest intensity of insolation and the time of highest temp • Also true for lowest intensity and temp

  20. Part 12. Measuring Temp and Heat • Temperature • Measures the average Kinetic Energy of molecules • Water • Celsius: 100º boils, 0º freezes • Fahrenheit: 212º boils, 32º freezes • Kelvin: 373 º boils, 273 º freezes, 0 º absolute zero • Absolute Zero • Coldest possible temp, molecules stop moving, no KE • -273º C, -459º F or 0º K

  21. Part 12. Measuring Temp and Heat • Heat • Measures the TOTAL amount of ALL Kinetic Energy in all molecules of substance • Measured in joules

  22. Part 12. Measuring Temp and Heat • Specific Heat • Amount of heat needed to raise one gram of a substance 1 º C • Specific Heat of Water = 4.18 joules/gºC • Lower the specific heat, the faster something will heat up or cool off.

  23. Part 13. States of Matter • Solids • Particles close together, definite shape • Liquids • Particles more separated, assumes shape of container • Gases • Particles farther apart than liquids

  24. Part 14. Changes of State • Melting • Solid to liquid • Needs heat energy that is stored as Potential Energy (no temp change) • Heat of Fusion – heat needed to change 1 gram of solid into liquid • HF for water = 334 Joules/g

  25. Part 14. Changes of State • Freezing (Fusion) • Liquid to solid • Heat is removed (given-off) • Use Heat of Fusion also

  26. Part 14. Changes of State • Vaporization (evaporation) • Liquid to gas • Needs heat energy that is stored as Potential Energy (no temp change) • Heat of Vaporization – heat needed to change 1 gram of liquid into gas • HV for water = 2260 Joules/g

  27. Part 14. Changes of State • Condensation • Gas to liquid • Heat is removed (given-off) • Use Heat of Vaporization also

  28. Part 14. Changes of State • Problems • How much heat is needed to change 20g of ice at 0 º C into 20g of water at 0 º C? Heat Energy (Q) = Mass (m) x HF Q = mHF Q = 20g x 334 J/g Q = 6680 Joules

  29. Part 14. Changes of State • How much heat must be lost to turn 50 g of water at 0 º C into ice at 0 º C ? Q = mHF Q = 50g x 334 J/g Q = 16700 Joules

  30. Part 14. Changes of State • How much energy is needed to turn 50g of water at 100 º C into 50g of steam at 100 º C ? Q = mHV Q = 50g x 2260 J/g Q = 113,000 Joules Which takes more energy melting ice or boiling water?

  31. What temp does this substance melt? • What temp does it boil? • At this rate, how long does it take to turn the substance from a solid at 40 º C into gas at 170 º C ?

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