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Ch23 change ofphase

This document discusses phase changes in matter such as evaporation, condensation, and boiling. It explains that evaporation occurs when molecules at the surface of a liquid gain enough kinetic energy to break free of the liquid as a gas. Condensation is the opposite change where gas molecules lose kinetic energy and stick together as a liquid. The rates of evaporation and condensation can be equal, resulting in no temperature change. Boiling occurs below the surface of a liquid when vapor pressure allows bubbles to form and rise. Pressure affects the boiling point temperature, with higher pressure requiring higher temperatures for boiling.

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23 Change of Phase Changes of phase usually involve a transfer of energy.
23 Change of Phase The four possible forms of matter—solid, liquid, gas, and plasma—are called phases. Matter can change from one phase to another. The phase of matter depends on its temperature and the pressure that is exerted upon it.
23 Change of Phase 23.1 Evaporation Evaporation is a process that cools the liquid left behind.
23 Change of Phase 23.1 Evaporation Water in an open container will eventually evaporate. The liquid that disappears becomes water vapor in the air. Evaporation is a change of phase from liquid to gas that takes place at the surface of a liquid.
23 Change of Phase 23.1 Evaporation Molecules in the liquid phase continuously move about in all directions and bump into one another at different speeds. Some of the molecules gain kinetic energy while others lose kinetic energy. Molecules at the surface of the liquid that gain kinetic energy may have enough energy to break free of the liquid. They now comprise a vapor, molecules in the gaseous phase.
23 Change of Phase 23.1 Evaporation The increased kinetic energy of molecules bumped free of the liquid comes from molecules remaining in the liquid. The average kinetic energy of the molecules remaining behind in the liquid is lowered.
23 Change of Phase 23.1 Evaporation The cloth covering on the sides of the canteen promotes cooling when it is wet. As the faster-moving water molecules leave the cloth, the temperature of the cloth decreases.
23 Change of Phase 23.1 Evaporation When the human body overheats, sweat glands produce perspiration. As the sweat evaporates, it cools us and helps us maintain a stable body temperature.
23 Change of Phase 23.1 Evaporation Pigs lack sweat glands. They wallow in mud to cool themselves.
23 Change of Phase 23.1 Evaporation How does evaporation affect a liquid’s temperature?
23 Change of Phase 23.2 Condensation Condensation warms the area where the liquid forms.
23 Change of Phase 23.2 Condensation Condensation is the changing of a gas to a liquid. Droplets form on a cold soda can when water vapor molecules collide with the slower-moving molecules of the cold can surface. The vapor molecules give up so much kinetic energy that they can’t stay in the gaseous phase. They condense.
23 Change of Phase 23.2 Condensation Condensation also occurs when gas molecules are captured by liquids. In their random motion, gas molecules may hit a liquid and lose kinetic energy. The attractive forces exerted on them by the liquid may hold them. Gas molecules become liquid molecules.
23 Change of Phase 23.2 Condensation Kinetic energy lost by condensing gas molecules warms the surface they strike. A steam burn is more damaging than a burn from boiling water because steam gives up energy when it condenses.
23 Change of Phase 23.2 Condensation Heat is given up by steam when it condenses inside the radiator.
23 Change of Phase 23.2 Condensation Relative Humidity At any given temperature and pressure, there is a limit to the amount of water vapor in the air. When any substance contains the maximum amount of another substance, the first substance is said to be saturated.
23 Change of Phase 23.2 Condensation The ratio between how much water vapor is in the air and the maximum amount that could be in the air at the same temperature is called the relative humidity. Relative humidity is not a measure of how much water vapor is in the air. In summer, with a low relative humidity, there may be more water vapor in the air than in winter with high relative humidity.
23 Change of Phase 23.2 Condensation At a relative humidity of 100%, the air is saturated. More water vapor is required to saturate high- temperature air than low-temperature air. The warm air of tropical regions is capable of containing much more moisture than cold Arctic air.
23 Change of Phase 23.2 Condensation For saturation, there must be water vapor molecules in the air undergoing condensation. When slow-moving molecules collide, some stick together— they condense. The faster the water molecules move, the less able they are to condense to form droplets.
23 Change of Phase 23.2 Condensation a. At high speeds, molecules of water vapor bounce apart and remain a gas.
23 Change of Phase 23.2 Condensation a. At high speeds, molecules of water vapor bounce apart and remain a gas. b. At lower speeds, molecules of water vapor are more likely to stick together and form a liquid.
23 Change of Phase 23.2 Condensation Temperature is a measure of average kinetic energy. There are always some molecules moving faster than average, and some moving slower. Even at high temperature, there will be enough slow molecules to cause condensation—provided there is enough water vapor.
23 Change of Phase 23.2 Condensation Fog and Clouds Warm air rises. As it rises, it expands. As it expands, it cools. As it cools, water vapor molecules begin sticking together after colliding, rather than bouncing off one another. If there are larger and slower-moving particles or ions present, water vapor condenses upon these particles, and makes a cloud.
23 Change of Phase 23.2 Condensation Fog is basically a cloud that forms near the ground. Fog occurs in areas where moist air near the ground cools. Some of the water vapor condenses out of the air as it cools, making fog. A key feature of fog and cloud formation is a slowing down of water vapor molecules in air.
23 Change of Phase 23.2 Condensation think! Is it correct to say that relative humidity is a measure of the amount of water vapor in the air at a particular temperature?
23 Change of Phase 23.2 Condensation think! Is it correct to say that relative humidity is a measure of the amount of water vapor in the air at a particular temperature? Answer: No. Humidity is a measure of the amount of water vapor per volume of air, whatever the temperature. Relative humidity, on the other hand, is the amount of vapor in the air compared with the amount for saturation at a particular temperature. Relative humidity is a ratio, expressed as a percent.
23 Change of Phase 23.2 Condensation How does condensation affect temperature?
23 Change of Phase 23.3 Evaporation and Condensation Rates The molecules and energy leaving a liquid’s surface by evaporation can be counteracted by as many molecules and as much energy returning by condensation.
23 Change of Phase 23.3 Evaporation and Condensation Rates When you emerge from a shower into a dry room, you often feel chilly because evaporation is taking place quickly. If you stay in the shower stall, moisture from the air condenses on your skin, counteracting the cooling of evaporation. If as much moisture condenses as evaporates, you will feel no change in body temperature.
23 Change of Phase 23.3 Evaporation and Condensation Rates If you leave a covered dish of water for several days, no apparent evaporation takes place. Much activity is taking place at the molecular level. Evaporation and condensation occur continuously at equal rates so the water level doesn’t change.
23 Change of Phase 23.3 Evaporation and Condensation Rates Evaporation and condensation normally take place at the same time. • If evaporation exceeds condensation, the liquid is cooled. • If condensation exceeds evaporation, the liquid is warmed.
23 Change of Phase 23.3 Evaporation and Condensation Rates How can evaporation and condensation take place at the same time?
23 Change of Phase 23.4 Boiling Increasing the pressure on the surface of a liquid raises the boiling point of the liquid.
23 Change of Phase 23.4 Boiling Evaporation takes place at the surface of a liquid. A change of phase from liquid to gas can also take place beneath the surface of a liquid, causing bubbles. The bubbles are buoyed upward to the surface, where they escape into the surrounding air. The change of phase from liquid to gas beneath a liquid’s surface is called boiling.
23 Change of Phase 23.4 Boiling The pressure of the vapor within the bubbles in a boiling liquid is great enough to resist the pressure of the surrounding water. Unless the vapor pressure is great enough, the surrounding pressures will collapse any bubbles that may form. Below the boiling point, the vapor pressure is not great enough. Bubbles do not form until the boiling point is reached.
23 Change of Phase 23.4 Boiling As the atmospheric pressure is increased, the molecules in the vapor must move faster to exert increased pressure to counteract the additional atmospheric pressure. At lowered pressure (as at high altitudes) boiling point decreases. Boiling depends not only on temperature but on pressure also.
23 Change of Phase 23.4 Boiling High Pressure A pressure cooker has a tight-fitting lid that does not allow vapor to escape until it reaches a certain pressure. As the vapor builds up inside the sealed pressure cooker, pressure on the surface of the liquid is increased, which prevents boiling. Increased pressure forces the water to reach a higher temperature before boiling can occur. The increased temperature of the water cooks the food faster.
23 Change of Phase 23.4 Boiling Low Pressure It is important to note that it is the high temperature of the water that cooks the food, not the boiling process itself. At high altitudes, water boils at a lower temperature. In Denver, water boils at 95°C, instead of the 100°C of sea level. If you try to cook food in boiling water of a lower temperature, you must wait a longer time for proper cooking.
23 Change of Phase 23.4 Boiling Boiling, like evaporation, is a process that cools the liquid. When 100°C water at atmospheric pressure is boiling, heat is taken away as fast as it is added. If cooling did not take place, continued application of heat to boiling water would result in a continued increase in temperature.
23 Change of Phase 23.4 Boiling think! Since boiling is a cooling process, would it be a good idea to cool your hot and sticky hands by dipping them into boiling water? Explain.
23 Change of Phase 23.4 Boiling think! Since boiling is a cooling process, would it be a good idea to cool your hot and sticky hands by dipping them into boiling water? Explain. Answer: No, no, no! When we say boiling is a cooling process, we mean that the water (not your hands!) is being cooled. A dip in 100°C water would be most uncomfortable for your hands!
23 Change of Phase 23.4 Boiling What is the effect of pressure on the boiling temperature of a liquid?
23 Change of Phase 23.5 Freezing In general, dissolving anything in a liquid lowers the liquid’s freezing temperature.
23 Change of Phase 23.5 Freezing When energy is continually withdrawn from a liquid, molecular motion slows. Eventually, the forces of attraction between the molecules cause them to get closer to one another. The molecules then vibrate about fixed positions and form a solid.
23 Change of Phase 23.5 Freezing When energy is extracted from water at a temperature of 0°C and at atmospheric pressure, ice is formed. The change in phase from liquid to solid is called freezing.
23 Change of Phase 23.5 Freezing If sugar or salt is dissolved in the water, the freezing temperature will be lowered. The molecules or ions get in the way of water molecules that otherwise would join into a six-sided ice-crystal structure. Antifreeze is a practical application of this process.
23 Change of Phase 23.5 Freezing Pure ice crystals have an open structure. When other kinds of molecules or ions are introduced, crystal formation is interrupted, and the freezing temperature is lowered.
23 Change of Phase 23.5 Freezing What effect does dissolving anything in a liquid have on the liquid’s freezing temperature?
23 Change of Phase 23.6 Boiling and Freezing at the Same Time Lowering the pressure can cause boiling and freezing to take place at the same time!
23 Change of Phase 23.6 Boiling and Freezing at the Same Time A dish of water at room temperature is placed in a vacuum jar. A gram or two of water is placed in a dish that is insulated from the base by a polystyrene cup.
23 Change of Phase 23.6 Boiling and Freezing at the Same Time • If the pressure in the jar is slowly reduced, the water will start to boil. • The boiling process takes higher-energy molecules away from the water left in the dish, which cools to a lower temperature.
23 Change of Phase 23.6 Boiling and Freezing at the Same Time • As the pressure is further reduced, more and more of the faster remaining slow-moving molecules boil away. • Continued boiling results in a lowering of temperature until the freezing point of approximately 0°C is reached. • Cooling by boiling causes ice to form over the bubbling water.
23 Change of Phase 23.6 Boiling and Freezing at the Same Time If drops of coffee are sprayed into a vacuum chamber, they, too, will boil until they freeze. Even after they are frozen, the water molecules will continue to evaporate until little crystals of coffee solids are left. This is how freeze-dried coffee is made. The low temperature of this process tends to keep the chemical structure of coffee solids from changing.
23 Change of Phase 23.6 Boiling and Freezing at the Same Time What can cause boiling and freezing to take place at the same time?
23 Change of Phase 23.7 Regelation Regelation can occur only in substances that expand when they freeze.
23 Change of Phase 23.7 Regelation The open-structured crystals of ice can be crushed by the application of pressure. Ice normally melts at 0°C, but pressure lowers the melting point. The crystals are simply crushed to the liquid phase. At twice standard atmospheric pressure, the melting point is lowered to -0.007°C.
23 Change of Phase 23.7 Regelation When the pressure is removed, refreezing occurs. The phenomenon of melting under pressure and freezing again when the pressure is reduced is called regelation. It is one of the properties of water that make it different from other substances.
23 Change of Phase 23.7 Regelation You can see regelation if you suspend a fine wire that supports heavy weights over an ice block. The wire will cut through the ice, but its track will refill with ice. The wire and weights fall to the floor, leaving the ice in a single solid piece!
23 Change of Phase 23.7 Regelation To make a snowball, you use regelation. When you compress the snow with your hands, you cause a slight melting, which helps to bind the snow into a ball. Making snowballs is difficult in very cold weather, because the pressure you can apply may not be enough to melt the snow.
23 Change of Phase 23.7 Regelation Why do so few substances undergo regelation?
23 Change of Phase 23.8 Energy and Changes of Phase Energy must be put into a substance to change its phase from solid to liquid to gas. Conversely, energy must be extracted from a substance to change its phase from gas to liquid to solid.
23 Change of Phase 23.8 Energy and Changes of Phase If you heat a solid sufficiently, it will melt and become a liquid. If you heat the liquid, it will vaporize and become a gas. The change in the internal energy of a substance causes the change of phase.
23 Change of Phase 23.8 Energy and Changes of Phase Examples of Phase Changes Suppose we have a 1-gram piece of ice at a temperature of -50°C in a closed container, and it is put on a stove to heat.
23 Change of Phase 23.8 Energy and Changes of Phase • A thermometer in the container reveals a slow increase in temperature up to 0°C. • Once it reaches 0°C, the temperature of the ice remains at 0°C even though heat input continues. • Rather than getting warmer, the ice melts.
23 Change of Phase 23.8 Energy and Changes of Phase • In order for the whole gram of ice to melt, 80 calories (335 joules) of heat energy must be absorbed by the ice. • Not until all the ice melts does the temperature again begin to rise.
23 Change of Phase 23.8 Energy and Changes of Phase • Each additional calorie absorbed by the gram of water increases its temperature by 1°C until it reaches its boiling temperature, 100°C.
23 Change of Phase 23.8 Energy and Changes of Phase • The temperature remains constant while water is boiled away. The water absorbs 540 calories (2255 joules) of heat to vaporize the gram. • When all the water has become steam at 100°C, the temperature begins to rise once more.
23 Change of Phase 23.8 Energy and Changes of Phase Reversibility of Phase Changes The phase change sequence is reversible. • When the molecules in a gram of steam condense to form water, they liberate 540 calories (2255 joules) of heat. • When the water is cooled from 100°C to 0°C, 100 additional calories are liberated to the environment. • When ice water fuses to become solid ice, 80 more calories (335 joules) of energy are released by the water.
23 Change of Phase 23.8 Energy and Changes of Phase The 540 calories (2255 joules) required to vaporize a gram of water is a relatively large amount of energy. It is much more than is required to change a gram of ice at absolute zero to boiling water at 100°C. Although the molecules in steam and boiling water at 100°C have the same average kinetic energy, steam has more potential energy.
23 Change of Phase 23.8 Energy and Changes of Phase In steam, the molecules are free of each other and are not bound together in the liquid. A vast amount of energy can be released during condensation.
23 Change of Phase 23.8 Energy and Changes of Phase Under some conditions hot water will freeze faster than warm water. This occurs for water hotter than 80°C. Cooling rates by rapid evaporation are very high. Each gram of water draws 540 calories from the water left behind. This is an enormous quantity of energy compared to cooling by thermal conduction.
23 Change of Phase 23.8 Energy and Changes of Phase When a car is washed on a cold day, hot water will freeze more readily than warm water because of the energy that the rapidly evaporating water takes with it.
23 Change of Phase 23.8 Energy and Changes of Phase Applications of Phase Changes A refrigerator’s cooling cycle uses the changes of phase of the refrigeration fluid (not water).
23 Change of Phase 23.8 Energy and Changes of Phase Applications of Phase Changes • Liquid is pumped into the cooling unit, where it is forced through a tiny opening to evaporate.
23 Change of Phase 23.8 Energy and Changes of Phase Applications of Phase Changes • It draws heat from the things stored in the food compartment.
23 Change of Phase 23.8 Energy and Changes of Phase Applications of Phase Changes • The gas then goes to coils located outside the cooling unit.
23 Change of Phase 23.8 Energy and Changes of Phase Applications of Phase Changes • As the gas condenses in the coils, heat is given off.
23 Change of Phase 23.8 Energy and Changes of Phase Applications of Phase Changes • The liquid returns to the cooling unit, and the cycle continues.
23 Change of Phase 23.8 Energy and Changes of Phase A motor pumps the fluid through the system, where it enters the cyclic processes of vaporization and condensation. Place your hand near the condensation coils of a refrigerator and you will feel the heat that has been extracted from the inside.
23 Change of Phase 23.8 Energy and Changes of Phase An air conditioner employs the same principles. It simply pumps heat from one part of the unit to another. When the roles of vaporization and condensation are reversed, the air conditioner becomes a heater. A device that moves heat is called a heat pump.
23 Change of Phase 23.8 Energy and Changes of Phase Some people judge the hotness of a clothes iron by touching it briefly with a finger. This is also a way to burn the finger—unless it is first moistened. Energy that ordinarily would go into burning the finger goes, instead, into changing the phase of the moisture on it.
23 Change of Phase 23.8 Energy and Changes of Phase • A solid absorbs energy when it melts. • A liquid absorbs energy when it vaporizes. • A gas emits energy when it liquefies. • A liquid releases energy when it solidifies.
23 Change of Phase 23.8 Energy and Changes of Phase think! How much energy is released when a gram of steam at 100°C condenses to water at 100°C?
23 Change of Phase 23.8 Energy and Changes of Phase think! How much energy is released when a gram of steam at 100°C condenses to water at 100°C? Answer: One gram of steam at 100°C releases 540 calories of energy when it condenses to become water at the same temperature.
23 Change of Phase 23.8 Energy and Changes of Phase think! When H2O in the vapor phase condenses, is the surrounding air warmed or cooled?
23 Change of Phase 23.8 Energy and Changes of Phase think! When H2O in the vapor phase condenses, is the surrounding air warmed or cooled? Answer: The surrounding air is warmed because the change of phase is from vapor to liquid, which releases energy.
23 Change of Phase 23.8 Energy and Changes of Phase How is energy related to phase changes?
23 Change of Phase Assessment Questions 1. When evaporation occurs, the molecules left behind in the water a. are more energetic. b. have increased average speeds. c. result in lowered temperature and decreased energy. d. have a higher temperature and are less energetic.
23 Change of Phase Assessment Questions 1. When evaporation occurs, the molecules left behind in the water a. are more energetic. b. have increased average speeds. c. result in lowered temperature and decreased energy. d. have a higher temperature and are less energetic. Answer: C
23 Change of Phase Assessment Questions 2. When relatively slow-moving molecules condense from the air, the temperature of the remaining air tends to a. remain unchanged. b. decrease. c. increase. d. spread out uniformly.
23 Change of Phase Assessment Questions 2. When relatively slow-moving molecules condense from the air, the temperature of the remaining air tends to a. remain unchanged. b. decrease. c. increase. d. spread out uniformly. Answer: C
23 Change of Phase Assessment Questions 3. Put a saucer of water on your table. A process that then occurs is a. evaporation. b. condensation. c. both of these d. neither of these
23 Change of Phase Assessment Questions 3. Put a saucer of water on your table. A process that then occurs is a. evaporation. b. condensation. c. both of these d. neither of these Answer: C
23 Change of Phase Assessment Questions 4. The process of boiling water tends to a. warm the water. b. cool the water. c. both warm and cool the water at the same time. d. have no effect on the water’s temperature.
23 Change of Phase Assessment Questions 4. The process of boiling water tends to a. warm the water. b. cool the water. c. both warm and cool the water at the same time. d. have no effect on the water’s temperature. Answer: B
23 Change of Phase Assessment Questions 5. When salt is introduced to water, the temperature at which freezing takes place is a. unaffected. b. lowered. c. increased. d. dependent on the shape of ice crystals.
23 Change of Phase Assessment Questions 5. When salt is introduced to water, the temperature at which freezing takes place is a. unaffected. b. lowered. c. increased. d. dependent on the shape of ice crystals. Answer: B
23 Change of Phase Assessment Questions 6. Boiling and freezing occur when water is subjected to a. decreased temperatures. b. decreased atmospheric pressure. c. increased temperatures. d. increased atmospheric pressure.
23 Change of Phase Assessment Questions 6. Boiling and freezing occur when water is subjected to a. decreased temperatures. b. decreased atmospheric pressure. c. increased temperatures. d. increased atmospheric pressure. Answer: B
23 Change of Phase Assessment Questions 7. Regelation occurs due to water’s a. high specific heat. b. open-structured ice crystals. c. high rate of expansion. d. slight tendency to freeze when temperature is lowered.
23 Change of Phase Assessment Questions 7. Regelation occurs due to water’s a. high specific heat. b. open-structured ice crystals. c. high rate of expansion. d. slight tendency to freeze when temperature is lowered. Answer: B
23 Change of Phase Assessment Questions 8. When water changes to steam, energy is a. absorbed by the water. b. released by the water. c. conserved as the phase change occurs. d. changed to a different form.
23 Change of Phase Assessment Questions 8. When water changes to steam, energy is a. absorbed by the water. b. released by the water. c. conserved as the phase change occurs. d. changed to a different form. Answer: A

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Ch23 change ofphase

  • 1.
    23 Change ofPhase Changes of phase usually involve a transfer of energy.
  • 2.
    23 Change ofPhase The four possible forms of matter—solid, liquid, gas, and plasma—are called phases. Matter can change from one phase to another. The phase of matter depends on its temperature and the pressure that is exerted upon it.
  • 3.
    23 Change ofPhase 23.1 Evaporation Evaporation is a process that cools the liquid left behind.
  • 4.
    23 Change ofPhase 23.1 Evaporation Water in an open container will eventually evaporate. The liquid that disappears becomes water vapor in the air. Evaporation is a change of phase from liquid to gas that takes place at the surface of a liquid.
  • 5.
    23 Change ofPhase 23.1 Evaporation Molecules in the liquid phase continuously move about in all directions and bump into one another at different speeds. Some of the molecules gain kinetic energy while others lose kinetic energy. Molecules at the surface of the liquid that gain kinetic energy may have enough energy to break free of the liquid. They now comprise a vapor, molecules in the gaseous phase.
  • 6.
    23 Change ofPhase 23.1 Evaporation The increased kinetic energy of molecules bumped free of the liquid comes from molecules remaining in the liquid. The average kinetic energy of the molecules remaining behind in the liquid is lowered.
  • 7.
    23 Change ofPhase 23.1 Evaporation The cloth covering on the sides of the canteen promotes cooling when it is wet. As the faster-moving water molecules leave the cloth, the temperature of the cloth decreases.
  • 8.
    23 Change ofPhase 23.1 Evaporation When the human body overheats, sweat glands produce perspiration. As the sweat evaporates, it cools us and helps us maintain a stable body temperature.
  • 9.
    23 Change ofPhase 23.1 Evaporation Pigs lack sweat glands. They wallow in mud to cool themselves.
  • 10.
    23 Change ofPhase 23.1 Evaporation How does evaporation affect a liquid’s temperature?
  • 11.
    23 Change ofPhase 23.2 Condensation Condensation warms the area where the liquid forms.
  • 12.
    23 Change ofPhase 23.2 Condensation Condensation is the changing of a gas to a liquid. Droplets form on a cold soda can when water vapor molecules collide with the slower-moving molecules of the cold can surface. The vapor molecules give up so much kinetic energy that they can’t stay in the gaseous phase. They condense.
  • 13.
    23 Change ofPhase 23.2 Condensation Condensation also occurs when gas molecules are captured by liquids. In their random motion, gas molecules may hit a liquid and lose kinetic energy. The attractive forces exerted on them by the liquid may hold them. Gas molecules become liquid molecules.
  • 14.
    23 Change ofPhase 23.2 Condensation Kinetic energy lost by condensing gas molecules warms the surface they strike. A steam burn is more damaging than a burn from boiling water because steam gives up energy when it condenses.
  • 15.
    23 Change ofPhase 23.2 Condensation Heat is given up by steam when it condenses inside the radiator.
  • 16.
    23 Change ofPhase 23.2 Condensation Relative Humidity At any given temperature and pressure, there is a limit to the amount of water vapor in the air. When any substance contains the maximum amount of another substance, the first substance is said to be saturated.
  • 17.
    23 Change ofPhase 23.2 Condensation The ratio between how much water vapor is in the air and the maximum amount that could be in the air at the same temperature is called the relative humidity. Relative humidity is not a measure of how much water vapor is in the air. In summer, with a low relative humidity, there may be more water vapor in the air than in winter with high relative humidity.
  • 18.
    23 Change ofPhase 23.2 Condensation At a relative humidity of 100%, the air is saturated. More water vapor is required to saturate high- temperature air than low-temperature air. The warm air of tropical regions is capable of containing much more moisture than cold Arctic air.
  • 19.
    23 Change ofPhase 23.2 Condensation For saturation, there must be water vapor molecules in the air undergoing condensation. When slow-moving molecules collide, some stick together— they condense. The faster the water molecules move, the less able they are to condense to form droplets.
  • 20.
    23 Change ofPhase 23.2 Condensation a. At high speeds, molecules of water vapor bounce apart and remain a gas.
  • 21.
    23 Change ofPhase 23.2 Condensation a. At high speeds, molecules of water vapor bounce apart and remain a gas. b. At lower speeds, molecules of water vapor are more likely to stick together and form a liquid.
  • 22.
    23 Change ofPhase 23.2 Condensation Temperature is a measure of average kinetic energy. There are always some molecules moving faster than average, and some moving slower. Even at high temperature, there will be enough slow molecules to cause condensation—provided there is enough water vapor.
  • 23.
    23 Change ofPhase 23.2 Condensation Fog and Clouds Warm air rises. As it rises, it expands. As it expands, it cools. As it cools, water vapor molecules begin sticking together after colliding, rather than bouncing off one another. If there are larger and slower-moving particles or ions present, water vapor condenses upon these particles, and makes a cloud.
  • 24.
    23 Change ofPhase 23.2 Condensation Fog is basically a cloud that forms near the ground. Fog occurs in areas where moist air near the ground cools. Some of the water vapor condenses out of the air as it cools, making fog. A key feature of fog and cloud formation is a slowing down of water vapor molecules in air.
  • 25.
    23 Change ofPhase 23.2 Condensation think! Is it correct to say that relative humidity is a measure of the amount of water vapor in the air at a particular temperature?
  • 26.
    23 Change ofPhase 23.2 Condensation think! Is it correct to say that relative humidity is a measure of the amount of water vapor in the air at a particular temperature? Answer: No. Humidity is a measure of the amount of water vapor per volume of air, whatever the temperature. Relative humidity, on the other hand, is the amount of vapor in the air compared with the amount for saturation at a particular temperature. Relative humidity is a ratio, expressed as a percent.
  • 27.
    23 Change ofPhase 23.2 Condensation How does condensation affect temperature?
  • 28.
    23 Change ofPhase 23.3 Evaporation and Condensation Rates The molecules and energy leaving a liquid’s surface by evaporation can be counteracted by as many molecules and as much energy returning by condensation.
  • 29.
    23 Change ofPhase 23.3 Evaporation and Condensation Rates When you emerge from a shower into a dry room, you often feel chilly because evaporation is taking place quickly. If you stay in the shower stall, moisture from the air condenses on your skin, counteracting the cooling of evaporation. If as much moisture condenses as evaporates, you will feel no change in body temperature.
  • 30.
    23 Change ofPhase 23.3 Evaporation and Condensation Rates If you leave a covered dish of water for several days, no apparent evaporation takes place. Much activity is taking place at the molecular level. Evaporation and condensation occur continuously at equal rates so the water level doesn’t change.
  • 31.
    23 Change ofPhase 23.3 Evaporation and Condensation Rates Evaporation and condensation normally take place at the same time. • If evaporation exceeds condensation, the liquid is cooled. • If condensation exceeds evaporation, the liquid is warmed.
  • 32.
    23 Change ofPhase 23.3 Evaporation and Condensation Rates How can evaporation and condensation take place at the same time?
  • 33.
    23 Change ofPhase 23.4 Boiling Increasing the pressure on the surface of a liquid raises the boiling point of the liquid.
  • 34.
    23 Change ofPhase 23.4 Boiling Evaporation takes place at the surface of a liquid. A change of phase from liquid to gas can also take place beneath the surface of a liquid, causing bubbles. The bubbles are buoyed upward to the surface, where they escape into the surrounding air. The change of phase from liquid to gas beneath a liquid’s surface is called boiling.
  • 35.
    23 Change ofPhase 23.4 Boiling The pressure of the vapor within the bubbles in a boiling liquid is great enough to resist the pressure of the surrounding water. Unless the vapor pressure is great enough, the surrounding pressures will collapse any bubbles that may form. Below the boiling point, the vapor pressure is not great enough. Bubbles do not form until the boiling point is reached.
  • 36.
    23 Change ofPhase 23.4 Boiling As the atmospheric pressure is increased, the molecules in the vapor must move faster to exert increased pressure to counteract the additional atmospheric pressure. At lowered pressure (as at high altitudes) boiling point decreases. Boiling depends not only on temperature but on pressure also.
  • 37.
    23 Change ofPhase 23.4 Boiling High Pressure A pressure cooker has a tight-fitting lid that does not allow vapor to escape until it reaches a certain pressure. As the vapor builds up inside the sealed pressure cooker, pressure on the surface of the liquid is increased, which prevents boiling. Increased pressure forces the water to reach a higher temperature before boiling can occur. The increased temperature of the water cooks the food faster.
  • 38.
    23 Change ofPhase 23.4 Boiling Low Pressure It is important to note that it is the high temperature of the water that cooks the food, not the boiling process itself. At high altitudes, water boils at a lower temperature. In Denver, water boils at 95°C, instead of the 100°C of sea level. If you try to cook food in boiling water of a lower temperature, you must wait a longer time for proper cooking.
  • 39.
    23 Change ofPhase 23.4 Boiling Boiling, like evaporation, is a process that cools the liquid. When 100°C water at atmospheric pressure is boiling, heat is taken away as fast as it is added. If cooling did not take place, continued application of heat to boiling water would result in a continued increase in temperature.
  • 40.
    23 Change ofPhase 23.4 Boiling think! Since boiling is a cooling process, would it be a good idea to cool your hot and sticky hands by dipping them into boiling water? Explain.
  • 41.
    23 Change ofPhase 23.4 Boiling think! Since boiling is a cooling process, would it be a good idea to cool your hot and sticky hands by dipping them into boiling water? Explain. Answer: No, no, no! When we say boiling is a cooling process, we mean that the water (not your hands!) is being cooled. A dip in 100°C water would be most uncomfortable for your hands!
  • 42.
    23 Change ofPhase 23.4 Boiling What is the effect of pressure on the boiling temperature of a liquid?
  • 43.
    23 Change ofPhase 23.5 Freezing In general, dissolving anything in a liquid lowers the liquid’s freezing temperature.
  • 44.
    23 Change ofPhase 23.5 Freezing When energy is continually withdrawn from a liquid, molecular motion slows. Eventually, the forces of attraction between the molecules cause them to get closer to one another. The molecules then vibrate about fixed positions and form a solid.
  • 45.
    23 Change ofPhase 23.5 Freezing When energy is extracted from water at a temperature of 0°C and at atmospheric pressure, ice is formed. The change in phase from liquid to solid is called freezing.
  • 46.
    23 Change ofPhase 23.5 Freezing If sugar or salt is dissolved in the water, the freezing temperature will be lowered. The molecules or ions get in the way of water molecules that otherwise would join into a six-sided ice-crystal structure. Antifreeze is a practical application of this process.
  • 47.
    23 Change ofPhase 23.5 Freezing Pure ice crystals have an open structure. When other kinds of molecules or ions are introduced, crystal formation is interrupted, and the freezing temperature is lowered.
  • 48.
    23 Change ofPhase 23.5 Freezing What effect does dissolving anything in a liquid have on the liquid’s freezing temperature?
  • 49.
    23 Change ofPhase 23.6 Boiling and Freezing at the Same Time Lowering the pressure can cause boiling and freezing to take place at the same time!
  • 50.
    23 Change ofPhase 23.6 Boiling and Freezing at the Same Time A dish of water at room temperature is placed in a vacuum jar. A gram or two of water is placed in a dish that is insulated from the base by a polystyrene cup.
  • 51.
    23 Change ofPhase 23.6 Boiling and Freezing at the Same Time • If the pressure in the jar is slowly reduced, the water will start to boil. • The boiling process takes higher-energy molecules away from the water left in the dish, which cools to a lower temperature.
  • 52.
    23 Change ofPhase 23.6 Boiling and Freezing at the Same Time • As the pressure is further reduced, more and more of the faster remaining slow-moving molecules boil away. • Continued boiling results in a lowering of temperature until the freezing point of approximately 0°C is reached. • Cooling by boiling causes ice to form over the bubbling water.
  • 53.
    23 Change ofPhase 23.6 Boiling and Freezing at the Same Time If drops of coffee are sprayed into a vacuum chamber, they, too, will boil until they freeze. Even after they are frozen, the water molecules will continue to evaporate until little crystals of coffee solids are left. This is how freeze-dried coffee is made. The low temperature of this process tends to keep the chemical structure of coffee solids from changing.
  • 54.
    23 Change ofPhase 23.6 Boiling and Freezing at the Same Time What can cause boiling and freezing to take place at the same time?
  • 55.
    23 Change ofPhase 23.7 Regelation Regelation can occur only in substances that expand when they freeze.
  • 56.
    23 Change ofPhase 23.7 Regelation The open-structured crystals of ice can be crushed by the application of pressure. Ice normally melts at 0°C, but pressure lowers the melting point. The crystals are simply crushed to the liquid phase. At twice standard atmospheric pressure, the melting point is lowered to -0.007°C.
  • 57.
    23 Change ofPhase 23.7 Regelation When the pressure is removed, refreezing occurs. The phenomenon of melting under pressure and freezing again when the pressure is reduced is called regelation. It is one of the properties of water that make it different from other substances.
  • 58.
    23 Change ofPhase 23.7 Regelation You can see regelation if you suspend a fine wire that supports heavy weights over an ice block. The wire will cut through the ice, but its track will refill with ice. The wire and weights fall to the floor, leaving the ice in a single solid piece!
  • 59.
    23 Change ofPhase 23.7 Regelation To make a snowball, you use regelation. When you compress the snow with your hands, you cause a slight melting, which helps to bind the snow into a ball. Making snowballs is difficult in very cold weather, because the pressure you can apply may not be enough to melt the snow.
  • 60.
    23 Change ofPhase 23.7 Regelation Why do so few substances undergo regelation?
  • 61.
    23 Change ofPhase 23.8 Energy and Changes of Phase Energy must be put into a substance to change its phase from solid to liquid to gas. Conversely, energy must be extracted from a substance to change its phase from gas to liquid to solid.
  • 62.
    23 Change ofPhase 23.8 Energy and Changes of Phase If you heat a solid sufficiently, it will melt and become a liquid. If you heat the liquid, it will vaporize and become a gas. The change in the internal energy of a substance causes the change of phase.
  • 63.
    23 Change ofPhase 23.8 Energy and Changes of Phase Examples of Phase Changes Suppose we have a 1-gram piece of ice at a temperature of -50°C in a closed container, and it is put on a stove to heat.
  • 64.
    23 Change ofPhase 23.8 Energy and Changes of Phase • A thermometer in the container reveals a slow increase in temperature up to 0°C. • Once it reaches 0°C, the temperature of the ice remains at 0°C even though heat input continues. • Rather than getting warmer, the ice melts.
  • 65.
    23 Change ofPhase 23.8 Energy and Changes of Phase • In order for the whole gram of ice to melt, 80 calories (335 joules) of heat energy must be absorbed by the ice. • Not until all the ice melts does the temperature again begin to rise.
  • 66.
    23 Change ofPhase 23.8 Energy and Changes of Phase • Each additional calorie absorbed by the gram of water increases its temperature by 1°C until it reaches its boiling temperature, 100°C.
  • 67.
    23 Change ofPhase 23.8 Energy and Changes of Phase • The temperature remains constant while water is boiled away. The water absorbs 540 calories (2255 joules) of heat to vaporize the gram. • When all the water has become steam at 100°C, the temperature begins to rise once more.
  • 68.
    23 Change ofPhase 23.8 Energy and Changes of Phase Reversibility of Phase Changes The phase change sequence is reversible. • When the molecules in a gram of steam condense to form water, they liberate 540 calories (2255 joules) of heat. • When the water is cooled from 100°C to 0°C, 100 additional calories are liberated to the environment. • When ice water fuses to become solid ice, 80 more calories (335 joules) of energy are released by the water.
  • 69.
    23 Change ofPhase 23.8 Energy and Changes of Phase The 540 calories (2255 joules) required to vaporize a gram of water is a relatively large amount of energy. It is much more than is required to change a gram of ice at absolute zero to boiling water at 100°C. Although the molecules in steam and boiling water at 100°C have the same average kinetic energy, steam has more potential energy.
  • 70.
    23 Change ofPhase 23.8 Energy and Changes of Phase In steam, the molecules are free of each other and are not bound together in the liquid. A vast amount of energy can be released during condensation.
  • 71.
    23 Change ofPhase 23.8 Energy and Changes of Phase Under some conditions hot water will freeze faster than warm water. This occurs for water hotter than 80°C. Cooling rates by rapid evaporation are very high. Each gram of water draws 540 calories from the water left behind. This is an enormous quantity of energy compared to cooling by thermal conduction.
  • 72.
    23 Change ofPhase 23.8 Energy and Changes of Phase When a car is washed on a cold day, hot water will freeze more readily than warm water because of the energy that the rapidly evaporating water takes with it.
  • 73.
    23 Change ofPhase 23.8 Energy and Changes of Phase Applications of Phase Changes A refrigerator’s cooling cycle uses the changes of phase of the refrigeration fluid (not water).
  • 74.
    23 Change ofPhase 23.8 Energy and Changes of Phase Applications of Phase Changes • Liquid is pumped into the cooling unit, where it is forced through a tiny opening to evaporate.
  • 75.
    23 Change ofPhase 23.8 Energy and Changes of Phase Applications of Phase Changes • It draws heat from the things stored in the food compartment.
  • 76.
    23 Change ofPhase 23.8 Energy and Changes of Phase Applications of Phase Changes • The gas then goes to coils located outside the cooling unit.
  • 77.
    23 Change ofPhase 23.8 Energy and Changes of Phase Applications of Phase Changes • As the gas condenses in the coils, heat is given off.
  • 78.
    23 Change ofPhase 23.8 Energy and Changes of Phase Applications of Phase Changes • The liquid returns to the cooling unit, and the cycle continues.
  • 79.
    23 Change ofPhase 23.8 Energy and Changes of Phase A motor pumps the fluid through the system, where it enters the cyclic processes of vaporization and condensation. Place your hand near the condensation coils of a refrigerator and you will feel the heat that has been extracted from the inside.
  • 80.
    23 Change ofPhase 23.8 Energy and Changes of Phase An air conditioner employs the same principles. It simply pumps heat from one part of the unit to another. When the roles of vaporization and condensation are reversed, the air conditioner becomes a heater. A device that moves heat is called a heat pump.
  • 81.
    23 Change ofPhase 23.8 Energy and Changes of Phase Some people judge the hotness of a clothes iron by touching it briefly with a finger. This is also a way to burn the finger—unless it is first moistened. Energy that ordinarily would go into burning the finger goes, instead, into changing the phase of the moisture on it.
  • 82.
    23 Change ofPhase 23.8 Energy and Changes of Phase • A solid absorbs energy when it melts. • A liquid absorbs energy when it vaporizes. • A gas emits energy when it liquefies. • A liquid releases energy when it solidifies.
  • 83.
    23 Change ofPhase 23.8 Energy and Changes of Phase think! How much energy is released when a gram of steam at 100°C condenses to water at 100°C?
  • 84.
    23 Change ofPhase 23.8 Energy and Changes of Phase think! How much energy is released when a gram of steam at 100°C condenses to water at 100°C? Answer: One gram of steam at 100°C releases 540 calories of energy when it condenses to become water at the same temperature.
  • 85.
    23 Change ofPhase 23.8 Energy and Changes of Phase think! When H2O in the vapor phase condenses, is the surrounding air warmed or cooled?
  • 86.
    23 Change ofPhase 23.8 Energy and Changes of Phase think! When H2O in the vapor phase condenses, is the surrounding air warmed or cooled? Answer: The surrounding air is warmed because the change of phase is from vapor to liquid, which releases energy.
  • 87.
    23 Change ofPhase 23.8 Energy and Changes of Phase How is energy related to phase changes?
  • 88.
    23 Change ofPhase Assessment Questions 1. When evaporation occurs, the molecules left behind in the water a. are more energetic. b. have increased average speeds. c. result in lowered temperature and decreased energy. d. have a higher temperature and are less energetic.
  • 89.
    23 Change ofPhase Assessment Questions 1. When evaporation occurs, the molecules left behind in the water a. are more energetic. b. have increased average speeds. c. result in lowered temperature and decreased energy. d. have a higher temperature and are less energetic. Answer: C
  • 90.
    23 Change ofPhase Assessment Questions 2. When relatively slow-moving molecules condense from the air, the temperature of the remaining air tends to a. remain unchanged. b. decrease. c. increase. d. spread out uniformly.
  • 91.
    23 Change ofPhase Assessment Questions 2. When relatively slow-moving molecules condense from the air, the temperature of the remaining air tends to a. remain unchanged. b. decrease. c. increase. d. spread out uniformly. Answer: C
  • 92.
    23 Change ofPhase Assessment Questions 3. Put a saucer of water on your table. A process that then occurs is a. evaporation. b. condensation. c. both of these d. neither of these
  • 93.
    23 Change ofPhase Assessment Questions 3. Put a saucer of water on your table. A process that then occurs is a. evaporation. b. condensation. c. both of these d. neither of these Answer: C
  • 94.
    23 Change ofPhase Assessment Questions 4. The process of boiling water tends to a. warm the water. b. cool the water. c. both warm and cool the water at the same time. d. have no effect on the water’s temperature.
  • 95.
    23 Change ofPhase Assessment Questions 4. The process of boiling water tends to a. warm the water. b. cool the water. c. both warm and cool the water at the same time. d. have no effect on the water’s temperature. Answer: B
  • 96.
    23 Change ofPhase Assessment Questions 5. When salt is introduced to water, the temperature at which freezing takes place is a. unaffected. b. lowered. c. increased. d. dependent on the shape of ice crystals.
  • 97.
    23 Change ofPhase Assessment Questions 5. When salt is introduced to water, the temperature at which freezing takes place is a. unaffected. b. lowered. c. increased. d. dependent on the shape of ice crystals. Answer: B
  • 98.
    23 Change ofPhase Assessment Questions 6. Boiling and freezing occur when water is subjected to a. decreased temperatures. b. decreased atmospheric pressure. c. increased temperatures. d. increased atmospheric pressure.
  • 99.
    23 Change ofPhase Assessment Questions 6. Boiling and freezing occur when water is subjected to a. decreased temperatures. b. decreased atmospheric pressure. c. increased temperatures. d. increased atmospheric pressure. Answer: B
  • 100.
    23 Change ofPhase Assessment Questions 7. Regelation occurs due to water’s a. high specific heat. b. open-structured ice crystals. c. high rate of expansion. d. slight tendency to freeze when temperature is lowered.
  • 101.
    23 Change ofPhase Assessment Questions 7. Regelation occurs due to water’s a. high specific heat. b. open-structured ice crystals. c. high rate of expansion. d. slight tendency to freeze when temperature is lowered. Answer: B
  • 102.
    23 Change ofPhase Assessment Questions 8. When water changes to steam, energy is a. absorbed by the water. b. released by the water. c. conserved as the phase change occurs. d. changed to a different form.
  • 103.
    23 Change ofPhase Assessment Questions 8. When water changes to steam, energy is a. absorbed by the water. b. released by the water. c. conserved as the phase change occurs. d. changed to a different form. Answer: A