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Thermal energy is transferred through the hydrosphere from warmer latitudes to cooler polar regions largely due to global winds.

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Presentation on theme: "Thermal energy is transferred through the hydrosphere from warmer latitudes to cooler polar regions largely due to global winds."— Presentation transcript:

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2 Thermal energy is transferred through the hydrosphere from warmer latitudes to cooler polar regions largely due to global winds.

3 The specific heat capacity is the amount of heat energy needed to raise the temperature of one gram of a substance by one degree celcius. The specific heat capacity of water is extremely large when compare to most other substances! Sweet.

4 A simple foam cup calorimeter. This is the amount of thermal energy that is released or absorbed by one gram of a substance when its temperature changes by one degree celcius. Q = thermal energy ( J ) m = mass ( g ) c = specific heat capacity ( J/g ºC ) Δt = change in temperature ( ºC )

5 1) A 350-g mass of water at 12.0ºC is allowed to warm up to 30.0ºC. Determine the amount of thermal energy, Q, absorbed. The theoretical specific heat capacity of water is 4.19 J/gºC x 10 4 J 2) Determine the quantity of energy required to warm a 2.00-kg block of ice from -25.0ºC to -10.0ºC. The theoretical specific heat capacity of ice is 2.00 J/gºC. Express your answer in kilojoules kJ

6 4) When 680 J of thermal energy is added to 30.0 g of iron, the temperature of the iron increases by 51.1ºC. What is the experimental specific heat capacity of iron? J/gºC 3) Calculate the change in temperature, Δt, that occurs when 30.0 kJ of thermal energy is added to 2.00 kg of copper. The theoretical specific heat capacity of copper is J/gºC. 39.0ºC

7 read pages 376 – 380 pages 379 – 380, Practice Problems #s 1 – 8 1) 1.51 × 10 4 J 2) 3.23 × 10 4 J 3) 1.26 × 10 3 J 4) 3.00 × 10 4 J 5) 20 ºC 6) water: 0.119ºC iron: 1.11ºC 7) J/gºC 8) J/gºC

8 (see text page 382)

9 During a phase change, the temperature of water remains constant. (text page 385)

10 The heat of fusion of a substance is the amount of energy released or absorbed when it changes from a liquid to a solid, or from a solid to a liquid. fusion solidification Q = thermal energy ( kJ ) H fus = heat of fusion ( kJ/mol ) n = number of moles of substance ( mol ) mass ( g ) molar mass ( g/mol )

11 The heat of vaporization of a substance is the amount of energy released or absorbed when it changes from a gas to a liquid, or from a liquid to a gas. vaporization condensation Q = thermal energy ( kJ ) H vap = heat of vaporization ( kJ/mol ) n = number of moles of substance ( mol )

12 1) When 4.18 kJ of thermal energy is added to 12.5 g of ice at its melting point, the ice changes phase. Given the molar mass of water is g/mol, calculate the experimental heat of fusion of ice kJ/mol 2) Calculate how much thermal energy is required to completely vaporize 30.0 g of liquid water, given that water has a molar mass of g/mol and the heat of vaporization of water is kJ/mol kJ

13 3) Determine the number of moles of silver at its melting point that can be melted by the addition of 50.0 kJ of energy, given that the heat of fusion of silver is kJ/mol mol

14 read pages 382 – 389 pages 386 – 387, Practice Problems #s 9 – 15 D2.3 Check and Reflect page 390 #s 1 – 2, 4, 6 – 8, 11 – 23 9) 6.01 kJ/mol 10) 19.2 kJ 11) 2.50 mol 12) kJ/mol 13) 3.48 kJ/mol 14) 40.7 kJ/mol 15) 1.13 × 10 3 kJ


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