3. C30S-1-04 Explain the process of melting, solidification, and deposition in C30S-1-05 terms of the KMT. Include: freezing point Use the KMT to explain evaporation and condensation
4. Energy Increased and Absorbed by Substance: SOLID to LIQUID Melting LIQUID to GAS Vaporization SOLID to GAS Sublimation GAS to PLASMA Ionization In all of these phase changes ENERGY IS ABSORBED . The initial state has a lower internal energy than the new state, so absorbs energy to change state. (A cooling process ) C30S-1-04 Explain the process of melting, solidification, and deposition in C30S-1-05 terms of the KMT. Include: freezing point Use the KMT to explain evaporation and condensation
5. Energy Decreased and Released by Substance: GAS to SOLID Deposition GAS to LIQUID Condensation LIQUID to SOLID Solidification PLASMA to GAS Deionization In all of these phase changes ENERGY IS RELEASED . The initial state has a greater internal energy than the new state, so releases energy to change state. (A warming process) C30S-1-04 Explain the process of melting, solidification, and deposition in C30S-1-05 terms of the KMT. Include: freezing point Use the KMT to explain evaporation and condensation
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8. Heating / Cooling Curves When a substance is heated, it undergoes several phase changes. A heating curve is a diagram that illustrates the phase changes that occur when a substance is heated. A cooling curve is a diagram that illustrates the phase changes that occur when a substance is cooled. C30S-1-04 Explain the process of melting, solidification, and deposition in C30S-1-05 terms of the KMT. Include: freezing point Use the KMT to explain evaporation and condensation
9. Heating / Cooling Curves C30S-1-04 Explain the process of melting, solidification, and deposition in C30S-1-05 terms of the KMT. Include: freezing point Use the KMT to explain evaporation and condensation
10. Heating / Cooling Curves Note that the melting and boiling processes require the addition of a specific amount of energy to break the forces holding the water molecules together. The temperature does not rise during the time of phase change because the energy is being used to change the phase of the material. When a liquid solidifies or condenses, the opposite occurs: energy is released and once again the temperature will remain constant. C30S-1-04 Explain the process of melting, solidification, and deposition in C30S-1-05 terms of the KMT. Include: freezing point Use the KMT to explain evaporation and condensation
19. Phase Changes - Animations C30S-1-04 Explain the process of melting, solidification, and deposition in C30S-1-05 terms of the KMT. Include: freezing point Use the KMT to explain evaporation and condensation
20. Phase Changes - Animations C30S-1-04 Explain the process of melting, solidification, and deposition in C30S-1-05 terms of the KMT. Include: freezing point Use the KMT to explain evaporation and condensation
21. Phase Changes - Animations C30S-1-04 Explain the process of melting, solidification, and deposition in C30S-1-05 terms of the KMT. Include: freezing point Use the KMT to explain evaporation and condensation
22. Vapour Pressure Design an Experiment C30S-1-06 Operationally define vapour pressure in terms of observable and measurable properties.
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25. Vapour Pressure C30S-1-06 Operationally define vapour pressure in terms of observable and measurable properties.
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28. Vapour Pressure Why do the 3 curves all look so different? C30S-1-06 Operationally define vapour pressure in terms of observable and C30S-1-07 measurable properties and operationally define normal boiling point in terms of vapour pressure.
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30. Determining The Normal Boiling Point of Various Substances C30S-1-07 Operationally define normal boiling point in terms of vapour pressure.
31. Determining The Normal Boiling Point of Various Substances C30S-1-07 Operationally define normal boiling point in terms of vapour pressure.
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33. Boiling Point Elevation When a solute is added to a solvent, the vapor pressure of the solvent (above the resulting solution) is less than the vapor pressure above the pure solvent. The boiling point of a solution, then, will be greater than the boiling point of the pure solvent because the solution (which has a lower vapor pressure) will need to be heated to a higher temperature in order for the vapor pressure to become equal to the external pressure (i.e., the boiling point). In other words from a molecular view we might expect the boiling point to be elevated when solute is increased in a solution.
34. Heat Effects in Changes of State Heat versus Temperature Heat is the measure of the quantity of energy in a system. Temperature is the measure of the intensity of that energy in the system "Given a bathtub full of water and a sink full of water, both having a temperature of 30°C, which will melt more ice cubes?"
35. Heat Effects in Changes of State Both have the same intensity of energy, or in other words, the same amount of thermal energy concentrated in each cm 3 of water. The water in the bathtub and sink, therefore, must have the same temperature. It is obvious, however, that more ice cubes would melt in the bathtub than the sink because the water in the bathtub contains a lot more energy or heat than the water in the sink.
36. Heat Effects in Changes of State Different instruments are needed to measure temperature and heat. A thermometer is used to measure temperature. A calorimeter is used to measure heat.
37. Heat can only be measured when energy is being transferred from one object to another. Temperature is measured by simply placing a thermometer in a substance and reading the intensity or concentration of the thermal energy in that substance. A calorimeter is used to measure the heat being transferred from one object having more energy (hot source) to an object having less energy (cold source).
38. Law of Heat Gain Temperature and heat are different, and are measured in different units. Temperature is measured in degrees Celsius (°C). Heat, like other energy forms, is measured in the S.I.. unit joule (J). An older unit of energy is the calorie. Dieticians still use the food Calorie (equal to 1000 calories).
39. Law of Heat Gain The relation between joules and calories is 1 cal = 4.184 J. 3 mini experiments
41. Law of Conservation of Heat The Law of Conservation of Energy states that in all reactions, energy is neither created nor destroyed. Analyzed in terms of the hot and cold water from the previous example, this means that the energy lost by the hot water was gained by the cold water. In other words, no energy was lost, it was simply transferred from one substance to another.
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43. What do you observe in the picture? Why do firefighters wear protective clothing?
44. Heat Capacity/Specific Heat Each material is able to "hold" a certain amount of thermal energy at a given temperature, due to what we call its specific heat . We have seen that the mass, the change in temperature, and the heat capacity (or specific heat) are all important in determining the quantity of heat lost or gained by a substance.
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46. The heat required to raise one gram of a substance by one degree Celsius is called ____. A. joule B. calorie C. specific heat D. energy
47. Heat Capacity/Specific Heat Mathematically they can be combined into q = m· T·C p q is the amount of heat lost or gained m is the mass C is the specific heat T is the change in temperature. Do Questions 4-6 on page 521 in your textbook. .
50. Measuring the Heat Capacity of a Metal Your assignment is to design an experiment and determine the heat capacity of a designated metal. You will be given an unknown metal and you must design an experiment to determine its heat capacity. Once the heat capacity is calculated, you will compare it against known values for certain metals to ascertain what metal it is.
53. Latent Heat When a substance changes phase, heat can be transferred in or out without any change in temperature. This occurs because of the energy required to change phase. What is happening is that the internal energy of the substance is changing, because the relationship between neighboring atoms and molecules changes.
54. Latent Heat The change in internal energy associated with a change in phase is known as the latent heat . It is called latent heat because there is no temperature change associated with this energy transfer, there is only a change in phase.
55. Latent Heat of Fusion & Vaporization For a liquid-solid phase change, it's called the latent heat of fusion . For a liquid-gas phase change, it's called the latent heat of vaporization .
58. ASSESSMENT C30S-1-03 Explain the properties of liquids and solids using the KMT.
Editor's Notes
Ethylene Glycol is an organic liquid called anti-freeze which is added to water to make an aqueous solution of Ethylene Glycol and water. This is to prevent water in the radiator of the vehicle from boiling over. It elevates the boiling point of water. At the same time, anti-freeze will depress the freezing point of that same water to prevent freeze up in the winter, hence the name of the solution, "anti-freeze". This ability for a solute to elevate the boiling point and depress the freezing point of the solvent is the focus of this page
Ethylene Glycol is an organic liquid called anti-freeze which is added to water to make an aqueous solution of Ethylene Glycol and water. This is to prevent water in the radiator of the vehicle from boiling over. It elevates the boiling point of water. At the same time, anti-freeze will depress the freezing point of that same water to prevent freeze up in the winter, hence the name of the solution, "anti-freeze". This ability for a solute to elevate the boiling point and depress the freezing point of the solvent is the focus of this page
Ethylene Glycol is an organic liquid called anti-freeze which is added to water to make an aqueous solution of Ethylene Glycol and water. This is to prevent water in the radiator of the vehicle from boiling over. It elevates the boiling point of water. At the same time, anti-freeze will depress the freezing point of that same water to prevent freeze up in the winter, hence the name of the solution, "anti-freeze". This ability for a solute to elevate the boiling point and depress the freezing point of the solvent is the focus of this page
Ethylene Glycol is an organic liquid called anti-freeze which is added to water to make an aqueous solution of Ethylene Glycol and water. This is to prevent water in the radiator of the vehicle from boiling over. It elevates the boiling point of water. At the same time, anti-freeze will depress the freezing point of that same water to prevent freeze up in the winter, hence the name of the solution, "anti-freeze". This ability for a solute to elevate the boiling point and depress the freezing point of the solvent is the focus of this page
(Heat always flows spontaneously from the hot source to the cold source.)
After completing the previous experiments, it should be evident that the heat "lost" from the candle is equal to the "heat" gained by the water, or that a constant fraction of the energy transferred goes to warm the water.
After completing the previous experiments, it should be evident that the heat "lost" from the candle is equal to the "heat" gained by the water, or that a constant fraction of the energy transferred goes to warm the water.
(Heat always flows spontaneously from the hot source to the cold source.)
the quantity of heat absorbed or lost is directly proportional to the mass. b. the quantity of heat absorbed or lost is directly proportional to change in temperature. c. the mass and change in temperature are inversely proportional. d. for every different substance there is a constant specific heat that does not vary.
After completing the previous experiments, it should be evident that the heat "lost" from the candle is equal to the "heat" gained by the water, or that a constant fraction of the energy transferred goes to warm the water.
Ethylene Glycol is an organic liquid called anti-freeze which is added to water to make an aqueous solution of Ethylene Glycol and water. This is to prevent water in the radiator of the vehicle from boiling over. It elevates the boiling point of water. At the same time, anti-freeze will depress the freezing point of that same water to prevent freeze up in the winter, hence the name of the solution, "anti-freeze". This ability for a solute to elevate the boiling point and depress the freezing point of the solvent is the focus of this page
Ethylene Glycol is an organic liquid called anti-freeze which is added to water to make an aqueous solution of Ethylene Glycol and water. This is to prevent water in the radiator of the vehicle from boiling over. It elevates the boiling point of water. At the same time, anti-freeze will depress the freezing point of that same water to prevent freeze up in the winter, hence the name of the solution, "anti-freeze". This ability for a solute to elevate the boiling point and depress the freezing point of the solvent is the focus of this page
Ethylene Glycol is an organic liquid called anti-freeze which is added to water to make an aqueous solution of Ethylene Glycol and water. This is to prevent water in the radiator of the vehicle from boiling over. It elevates the boiling point of water. At the same time, anti-freeze will depress the freezing point of that same water to prevent freeze up in the winter, hence the name of the solution, "anti-freeze". This ability for a solute to elevate the boiling point and depress the freezing point of the solvent is the focus of this page
Ethylene Glycol is an organic liquid called anti-freeze which is added to water to make an aqueous solution of Ethylene Glycol and water. This is to prevent water in the radiator of the vehicle from boiling over. It elevates the boiling point of water. At the same time, anti-freeze will depress the freezing point of that same water to prevent freeze up in the winter, hence the name of the solution, "anti-freeze". This ability for a solute to elevate the boiling point and depress the freezing point of the solvent is the focus of this page
A pure substance is matter in which the particles that make it up are all of the same kind. A mixture contains more than one kind of particle. In mixtures, the individual components of the mixture retain their properties. For example, water is a pure substance if it only contains water molecules, but tap water is a mixture because it contains added chlorine, fluorine, dissolved air and sometimes other things like bacteria and metals we are not happy about. Pure substances can be in the form of elements or compounds. Elements are called the building blocks of matter, since they contain only on type of atom. Compounds are pure substances that contain two or more different atoms joined chemically. We call this chemical joining a chemical bond. Mixtures can be heterogeneous and homogeneous. The particles in a heterogeneous mixture are not evenly distributed and individual particles are often distinguishable. For example, a mixture of sand and water or salt and pepper are heterogeneous. The individual particles of a homogeneous mixture are evenly distributed and cannot be easily separated. For example, when solid sugar is dissolved in water, only a liquid is observed and the solid sugar particles are not visible.
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