1 / 37

Science 10 – Hydrologic Cycle and Heat Capacity

Science 10 – Hydrologic Cycle and Heat Capacity. Objectives. Define specific heat capacity and use it to calculate thermal energy Describe the hydrological cycle Distinguish between different phases of the hydrological cycle Calculate heat of fusion and heat of vaporization. Planet Water.

mala
Download Presentation

Science 10 – Hydrologic Cycle and Heat Capacity

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Science 10 – Hydrologic Cycle and Heat Capacity

  2. Objectives • Define specific heat capacity and use it to calculate thermal energy • Describe the hydrological cycle • Distinguish between different phases of the hydrological cycle • Calculate heat of fusion and heat of vaporization

  3. Planet Water • 70% of Earth’s surface is covered with water • Water plays a major role in the absorption and distribution of thermal energy, influencing both weather and climate: the great moderator

  4. Hydrological Cycle • Water is constantly moving through the biosphere • Changing phases from solid to liquid to gas and back again • Uses evaporation, condensation, transpiration, and precipitation • Add or release thermal energy for phase changes

  5. How Oceans Effect Distribution of Heat Large Reservoirs of Heat • Water has high specific heat capacity • Water has low albedo, high absorption (90% of incoming solar radiation is absorbed

  6. Large Reservoirs of Heat • 3. High heats of fusion and vaporization • 4. Water is a fluid and heat can be distributed

  7. Areas around large bodies of water (Great Lakes, oceans) do not experience extreme weather changes like areas that don’t have large bodies of water i.e continent interiors (think Saskatchewan and Alberta), and deserts.

  8. Large bodies of water MODERATE temperature and climate. • It takes a lot of solar radiation to heat water, so water is a heat sink. • It absorbs a great deal of solar radiation, keeping the region cooler during the day, and it slowly reradiates the heat at night

  9. Ocean Currents • Large effect on weather in coastal communities • Influence worldwide climate

  10. Gulf Stream • Surface current: starts in Caribbean and flows up the Eastern coastline of US and Canada up to British Isles. Also called North Atlantic Drift.

  11. Huge air and ocean currents distribute heat in amazing patterns around the earth, greatly affecting the climate and weather of many regions.

  12. Phase Changes and Global Energy Transfer • Phase changes in the hydrologic cycle play a role in global transfer of thermal energy • The transfer of energy warms the air, which rises • This can cause thunderstorms or hurricanes

  13. How does all this affect weather and climate? • Different specific heat capacities (we will get to this in a minute) of the Earth’s different surfaces (sand, water, forests, etc) affect how much they heat up the air and water around them.

  14. How does this affect our weather and climate? • The Earth’s water absorbs a lot of heat from the surroundings when condensing, and it releases a lot of heat when it is evaporating.

  15. If you think of all the water that is condensing or evaporating all over the lakes, ponds, streams, oceans and clouds that’s a lot of heating and cooling!

  16. Energy Transfer Types • Heat of fusion • Energy absorbed when 1 mol of a substance changes from solid to liquid • Heat of Solidification • Energy released when 1 mol of a substance changes from liquid to solid • Heat of Vaporization • Energy absorbed when 1 mol of a substance changes from liquid to vapor

  17. Energy Transfer Types cont… • Heat of Condensation • Energy released when 1 mol of a substance changes from vapor to liquid • Which ones are endothermic? Exothermic?

  18. Specific Heat Capacity • Symbolized as “c” • Amount of energy needed to raise temp of 1 g of a substance by 1 degree Celsius • Water c= 4.19 J/g degree Celsius • This is high • What effect might this have on the climate of Vancouver compared to Calgary?

  19. Specific heat capacity is a constant and is represented by “c” Pg. 375

  20. Formula Q = mcΔT c = specific heat capacity J/goC ΔT = change in temperature oC m = mass g Q = amount of heat J If data are given in initial (T1) and final (T2) temperatures instead of change in temperature, calculate ΔT using ΔT = T2 – T1

  21. THE EFFECTS OF SPECIFIC HEAT CAPACITY ON THE EARTH’S WEATHER AND CLIMATE • a) The Earth’s land or water surface heats up as it absorbs solar radiation. • b) This thermal energy is transferred by conduction to surrounding cooler air or water causing convection currents in air and water

  22. Convection (transfer of thermal energy in fluids – liquids or gases) Convection currents – air circulates and distributes heat (remember warm air is less dense, rises, cooler air descends and takes its place close to the ground, it heats up…etc.

  23. Practice • A 50.0 g mass of water at 25.0 °C is heated to 50.0°C on a hot plate. Given that the theoretical specific heat capacity of water is 4.19 J/g°C, determine the value for Q • Answer: 5.24 J

  24. Practice • How much thermal energy must be released to decrease the temperature of 1.00 kg of water by 10.0 °C, given that the theoretical specific heat capacity of water is 4.19 J/g°C? • Answer: 41.9 kJ

  25. Practice • When 21.6 J of thermal energy is added to a 2.0 g mass of iron, the temperature of the iron increases by 24.0°C. What is the experimental specific heat capacity of iron? • 0.45 J/g°C

  26. Heat of Fusion, Heat of Vaporization: Phase Changes of Water Why is the ice and water absorbing energy with no change in temperature?

  27. Calculations Energy required for melting Energy required for vaporizing • Q = nHfusQ = nHvap • Q amount of heat energy J (joules) • n number of moles (no units) • Hfus heat of fusion J/mol • Hvap heat of vaporization J/mol

  28. Energy Transfer Graph Where on the graph would we label heat of fusion? Heat of vaporization?

  29. Calculating Heat of Fusion Hfus = _Q_ n Hfus= heat of fusion (kJ/mol) Q = quantity of thermal energy (kJ) n = amount of the substance (mol)

  30. Practice • When 27.05 kJ of thermal energy is added to 4.50 mol of ice at 0.0°C, the ice melts completely. What is the experimental heat of fusion of water? • Answer: 6.01 kJ/mol

  31. Practice • When 5.00 g of ice melts, 1.67 kJ of thermal energy is absorbed. Calculate the experimental heat of fusion of ice. The molar mass, M, of ice is 18.02 g/mol. • Answer: 6.0 kJ/mol

  32. Practice • When 0.751 kJ of thermal energy is added to 0.125 mol of ice at 0.0°C, the ice changes phase. Calculate the experimental heat of fusion of ice.

  33. Calculating Heat of Vaporization Hvap = _Q_ n Hvap = heat of vaporization (kJ/mol) Q = quantity of thermal energy (kJ/mol) n = amount of the substance (mol)

  34. Practice • When 150 g of water changes from liquid to vapor phase, 339 kJ of energy is absorbed. Determine the experimental heat of vaporization of water, given that the molar mass, M, of water is 18.02 g/mol • Answer: 40.7 kJ/mol

  35. Practice • When 8.70 kJ of thermal energy is added to 2.50 mol of liquid methanol, all the methanol enters the vapor phase. Determine the experimental heat of vaporization of methanol.

  36. Assignment • Specific Heat Practice problems # 1-8 pg. 379 • Pg 386/387, try practice problems

More Related