Agenda 1) Homework Questions 2) Review Concepts of Thermal Energy 3) States of Matter / Latent Heat 4) Practice
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1 Agenda 1) Homework Questions 2) Review Concepts of Thermal Energy 3) States of Matter / Latent Heat 4) Practice
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3 Important Terms and their Usage Drag each term below into the sentence in which it is properly used. Section Rubbing my hands together causes an increase in kinetic energy and makes them heat up. 2. thermal energy is the sum of both kinetic and potential energy in the atoms or molecules of a substance. 3. The Kelvin temperature scale is based on absolute zero, the temperature at which the atoms of all substances stop moving. 4. Measurement of temperature in Celcius is based on a scale that includes the freezing and boiling points of water. 5. For most substances, the melting point is the same as the freezing point. 6. The temperature at which a gas changes into a liquid is called the condensation point for the substance. Check Answer
4 Thermal Energy and Temperature Section 6.2 Which statements about the thermal energy and temperature of the two nails shown are true and which are false? Use the Line tool to cross out false statements and use the Highlight tool to mark true ones. Two nails with equal mass, with the same thermal energy, and made from the same material will not have the same temperature. Two nails with equal mass, with the same temperature, and made from the same material must have the same thermal energy. If the thermal energy of two nails made of the same material but with different masses is the same, they must have different temperatures. If the temperature of two nails made of the same material but with different masses is the same, they must have the same thermal energy. Check Answer
5 Heat Capacity Section 6.3 Which material will cool to a lower temperature when a given amount of energy is removed from it? Find the final temperature, in degrees Celsius, of 100 g of two materials water and lead after being cooled from 323 K to extract an equal amount of energy (1000 J) from each. First, rearrange the equation for the quantity of heat to solve for the final temperature. Solution: Q = mc T Q = mc(t 2 T 1 ) Q = mct 2 mct 1 mct 2 = mct 1 + Q T 2 = Next, calculate the starting temperature for each material in Celsius. T C = T K 273 T C = 273 T C = Check Answer
6 Heat Capacity Final temperature for water = T 2 = T 1 + Q / (m c water ) Section 6.3 Now find the final temperature, in degrees Celsius, of 100 g each of water and lead, when they begin at 50 C and 1000 J is removed. Reference data for heat capacity for each material is given: Specific heat capacity c water = 4.18 x 10 3 J kg C Specific heat capacity c lead = 1.3 x 10 2 J kg C = + / ( ) = + Discussion = C Final temperature for lead = T 2 = T 1 + Q / (m c lead ) = + / ( ) = + = C Check Answer
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8 States of Matter and Changes of State Section 6.4 Drag the events listed to correctly label the cooling curve of water. Cooling Graph for Water Condensation point of water vapour Freezing point of water Temperature Water vapour cooling down 60 Water vapour 50 condensing into liquid water Liquid water cooling down Thermal energy released Liquid water freezing into ice Ice cooling down Check Answer
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11 Water: A Special Liquid Most substances become denser than their liquid state as soon as they solidify at the point of freezing. This is not the case for the most common liquid on Earth, water. The structure of water molecules causes them to be disorganized when packed together above 4 C. This makes liquid water denser than solid ice. Section 6.4 Discussion What shape do water molecules form when they freeze into ice? HEXAGON Click Here!
12 ANSWERS ANSWERS TEACHER'S FOR THE TEACHER NOTES LESSON
13 Important Terms and their Usage Drag each term below into the sentence in which it is properly used. Section Rubbing my hands together causes an increase in kinetic energy and makes them heat up. 2. thermal energy is the sum of both kinetic and potential energy in the atoms or molecules of a substance. 3. The Kelvin temperature scale is based on absolute zero, the temperature at which the atoms of all substances stop moving. 4. Measurement of temperature in Celcius is based on a scale that includes the freezing and boiling points of water. 5. For most substances, the melting point is the same as the freezing point. 6. The temperature at which a gas changes into a liquid is called the condensation point for the substance. Back
14 Thermal Energy and Temperature Section 6.2 Which statements about the thermal energy and temperature of the two nails shown are true and which are false? Use the Line tool to cross out false statements and use the Highlight tool to mark true ones. Two nails with equal mass, with the same thermal energy, and made from the same material will not have the same temperature. Two nails with equal mass, with the same temperature, and made from the same material must have the same thermal energy. If the thermal energy of two nails made of the same material but with different masses is the same, they must have different temperatures. If the temperature of two nails made of the same material but with different masses is the same, they must have the same thermal energy. Back
15 Heat Capacity Section 6.3 Which material will cool to a lower temperature when a given amount of energy is removed from it? Find the final temperature, in degrees Celsius, of 100 g of two materials water and lead after being cooled from 323 K to extract an equal amount of energy (1000 J) from each. First, rearrange the equation for the quantity of heat to solve for the final temperature. Solution: Q = mc T Q = mc(t 2 T 1 ) Q = mct 2 mct 1 mct 2 = mct 1 + Q T 2 = Q/(mc) T 1 Next, calculate the starting temperature for each material in Celsius. T C = T K 273 T C = 323 K 273 T C = 50.0 C Back
16 Heat Capacity Section 6.3 Now find the final temperature, in degrees Celsius, of 100 g each of water and lead, when they begin at 50 C and 1000 J is removed. Reference data for heat capacity for each material is given: Specific heat capacity c water = 4.18 x 10 3 J kg C Specific heat capacity c lead = 1.3 x 10 2 J kg C Final temperature for water = T 2 = T 1 + Q / (m c water ) 4180 J = 50 C J / ( 0.1 kg kg C ) = 50 C + 2 C = 48 C Discussion Final temperature for lead = T 2 = T 1 + Q / (m c lead ) 130 J = 50 C J / ( 0.1 kg kg C ) = 50 C + 80 C = 30 C Back
17 States of Matter and Changes of State Section 6.4 Drag the events listed to correctly label the cooling curve of water. Cooling Graph for Water Condensation point of water vapour Freezing point of water Temperature Water vapour 80cooling down Water vapour condensing into liquid water Liquid water cooling down Thermal energy released Liquid water freezing into ice Ice cooling down Back
18 Answers for Discussion Questions: Slide 8 Sample answer: The difference in the change of temperature for the water vs. that of the lead is proportional to the ratio of the heat capacities of the two materials. Back
19 Answers for Discussion Questions: Slide 10 Sample answer: Some positive implications: Pipes in homes and underground would not burst if the water inside became cold enough to freeze. Icebergs that drift on the oceans near the North and South poles would sink below the surface and not threaten ships. Some negative implications: Aquatic life would be seriously threatened due to ice sinking to the bottom of lakes and oceans near the poles. This would significantly reduce the amount of oxygen produced in the oceans. The lack of Arctic ice would have serious implications for global warming because ice reflects much more sunlight back into space than water does. Back
20 Answers for Discussion Questions: Slide 12 Sample answer: Some advantages are as follows: The same system can provide both heating and cooling. Low operating cost compared to a furnace or hot water heating system. Thermal energy is plentiful and available for all to use. No risk of accidents involving explosions from propane or natural gas. Some disadvantages are as follows: Expensive to install, especially if the house is already built. Electricity is still required to operate the pump that moves the liquid anti freeze mixture through the plastic pipes. Leaks in the underground plastic piping may develop over time, causing antifreeze to be lost to the environment. Back
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