{"id":728,"date":"2018-03-20T15:40:28","date_gmt":"2018-03-20T15:40:28","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-orgbiochemistry\/?post_type=chapter&p=728"},"modified":"2018-08-14T20:10:40","modified_gmt":"2018-08-14T20:10:40","slug":"7-3-phase-changes","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/chapter\/7-3-phase-changes\/","title":{"raw":"7.3 Phase Changes","rendered":"7.3 Phase Changes"},"content":{"raw":"
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Learning Objectives<\/h3>\r\n
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  1. Determine the heat associated with a phase change.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\nDepending on the surrounding conditions, normal matter usually exists as one of three <\/span>phases<\/em>: solid, liquid, or gas.<\/span>\r\n\r\n<\/div>\r\n<\/div>\r\n
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    A phase change\u00a0<\/span><\/strong><\/span>is a physical process in which a substance goes from one phase to another. Usually the change occurs when adding or removing heat at a particular temperature, known as the melting point or the boiling point of the substance. The melting point<\/span><\/strong><\/span>\u00a0is the temperature at which the substance goes from a solid to a liquid, and it is exactly the same temperature as the\u00a0freezing point<\/strong>, the temperature at which a substance goes from a liquid to a solid). The boiling point<\/span><\/strong><\/span>\u00a0is the temperature at which a substance goes from a liquid to a gas at normal atmospheric pressure. The nature of the phase change depends on the direction of the heat transfer. Heat going into<\/em> a substance changes it from a solid to a liquid or a liquid to a gas. Removing heat from<\/em> a substance changes a gas to a liquid or a liquid to a solid.\u00a0 Adding energy to molecules makes them more faster and become more disorderly.\u00a0 Removing energy from molecules makes them slow down and become more orderly.<\/p>\r\n

    Two key points are worth emphasizing. First, at a substance\u2019s melting point or boiling point, two phases can exist simultaneously. Take water (H2<\/sub>O) as an example. On the Celsius scale, H2<\/sub>O has a melting point of 0\u00b0C and a boiling point of 100\u00b0C. At 0\u00b0C, both the solid and liquid phases of H2<\/sub>O can coexist. However, if heat is added, some of the solid H2<\/sub>O will melt and turn into liquid H2<\/sub>O. If heat is removed, the opposite happens: some of the liquid H2<\/sub>O turns into solid H2<\/sub>O. A similar process can occur at 100\u00b0C: adding heat increases the amount of gaseous H2<\/sub>O, while removing heat increases the amount of liquid H2<\/sub>O.<\/p>\r\n\r\n

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    Note<\/span><\/p>\r\n\r\n

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    Water is a good substance to use as an example because many people are already familiar with it. Other substances have melting points and boiling points as well.<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n

    Second, the temperature of a substance does not change as the substance goes from one phase to another. In other words, phase changes are isothermal,\u00a0<\/span><\/strong>which<\/span><\/span> means \u201cconstant temperature\u201d). Again, consider H2<\/sub>O as an example. Solid water (ice) can exist at 0\u00b0C. If heat is added to ice at 0\u00b0C, some of the solid changes phase to make liquid, which is also at 0\u00b0C. Remember, the solid and liquid phases of H2<\/sub>O can coexist at 0\u00b0C. Only after all of the solid has melted into liquid does the addition of heat change the temperature of the substance.<\/p>\r\n

    For each phase change of a substance, there is a characteristic quantity of heat needed to perform the phase change per gram (or per mole) of material. The heat of fusion<\/span><\/strong><\/span>\u00a0(\u0394H<\/em>fus<\/sub>) is the amount of heat per gram (or per mole) required for a phase change that occurs at the melting point. The heat of vaporization<\/span><\/strong><\/span>\u00a0(\u0394H<\/em>vap<\/sub>) is the amount of heat per gram (or per mole) required for a phase change that occurs at the boiling point. If you know the total number of grams or moles of material, you can use the \u0394H<\/em>fus<\/sub> or the \u0394H<\/em>vap<\/sub> to determine the total heat being transferred for melting or solidification using these expressions:<\/p>\r\nheat = n<\/em> \u00d7 \u0394H<\/em>fus<\/sub> (where n<\/em> is the number of moles)<\/span><\/span>\r\nor<\/span><\/span>\r\nheat = m<\/em> \u00d7 \u0394H<\/em>fus<\/sub> (where m<\/em> is the mass in grams)<\/span><\/span>\r\n

    For the boiling or condensation, use these expressions:<\/p>\r\nheat = n<\/em> \u00d7 \u0394H<\/em>vap<\/sub> (where n<\/em> is the number of moles)<\/span><\/span>\r\nor<\/span><\/span>\r\nheat = m<\/em> \u00d7 \u0394H<\/em>vap<\/sub> (where m<\/em> is the mass in grams)<\/span><\/span>\r\n

    Remember that a phase change depends on the direction of the heat transfer. If heat transfers in, solids become liquids, and liquids become solids at the melting and boiling points, respectively. If heat transfers out, liquids solidify, and gases condense into liquids.<\/p>\r\n\r\n

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    Example 4<\/h3>\r\n

    How much heat is necessary to melt 55.8 g of ice (solid H2<\/sub>O) at 0\u00b0C? The heat of fusion of H2<\/sub>O is 79.9 cal\/g.<\/p>\r\n

    Solution<\/p>\r\n

    We can use the relationship between heat and the heat of fusion to determine how many joules of heat are needed to melt this ice:<\/p>\r\nheat = m<\/em> \u00d7 \u0394H<\/em>fus<\/sub><\/span><\/span>\r\n heat\u00a0=\u00a0(55.8\u00a0g)(79.9[latex]\\frac{\\text{cal}}{\\text{g}}[\/latex])=4,460\u00a0cal <\/span>\r\n\r\n<\/div>\r\n

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    Skill-Building Exercise<\/h3>\r\n
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      How much heat is necessary to vaporize 685 g of H2<\/sub>O at 100\u00b0C? The heat of vaporization of H2<\/sub>O is 540 cal\/g.<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n \r\n\r\n<\/div>\r\n

      Table 7.4 \"Heats of Fusion and Vaporization for Selected Substances\"<\/a> lists the heats of fusion and vaporization for some common substances. Note the units on these quantities; when you use these values in problem solving, make sure that the other variables in your calculation are expressed in units consistent with the units in the specific heats or the heats of fusion and vaporization.<\/p>\r\n\r\n

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      Table 7.4<\/span> Heats of Fusion and Vaporization for Selected Substances<\/strong><\/h5>\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n
      Substance<\/th>\r\n\u0394H<\/em>fus<\/sub> (cal\/g)<\/th>\r\n\u0394H<\/em>vap<\/sub> (cal\/g)<\/th>\r\n<\/tr>\r\n<\/thead>\r\n
      aluminum (Al)<\/td>\r\n94.0<\/td>\r\n2,602<\/td>\r\n<\/tr>\r\n
      gold (Au)<\/td>\r\n15.3<\/td>\r\n409<\/td>\r\n<\/tr>\r\n
      iron (Fe)<\/td>\r\n63.2<\/td>\r\n1,504<\/td>\r\n<\/tr>\r\n
      water (H2<\/sub>O)<\/td>\r\n79.9<\/td>\r\n540<\/td>\r\n<\/tr>\r\n
      sodium chloride (NaCl)<\/td>\r\n123.5<\/td>\r\n691<\/td>\r\n<\/tr>\r\n
      ethanol (C2<\/sub>H5<\/sub>OH)<\/td>\r\n45.2<\/td>\r\n200.3<\/td>\r\n<\/tr>\r\n
      benzene (C6<\/sub>H6<\/sub>)<\/td>\r\n30.4<\/td>\r\n94.1<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n
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      Looking Closer: Sublimation and deposition<\/h3>\r\n

      There is also a phase change where a solid goes directly to a gas:<\/p>\r\n

      solid \u2192 gas\u00a0\u00a0 (sublimation)<\/strong>\r\n<\/span><\/span><\/p>\r\n

      We encounter sublimation in several ways. You may already be familiar with dry ice, which is simply solid carbon dioxide (CO2<\/sub>). At \u221278.5\u00b0C, solid carbon dioxide sublimes, changing directly from the solid phase to the gas phase:<\/p>\r\n

      CO2<\/sub>(s)\u00a0\u00a0\u2192\u00a0 CO2<\/sub>(g)\u00a0 at \u221278.5\u00b0C\r\n<\/span><\/p>\r\n

      Solid carbon dioxide is called dry<\/em> ice because it does not pass through the liquid phase but goes directly to the gas phase at normal atmospheric pressure. Dry ice has many practical uses, including the long-term preservation of medical samples.<\/p>\r\n

      Even plain old ice, solid H2<\/sub>O, slowly sublimes at temperatures below 0\u00b0C. For example, ice cubes in a freezer may get smaller over time. Although frozen, the solid water slowly sublimes, releasing water molecules into the air in the freezer. Water also sublimes from frozen foods, giving them an unattractive, mottled appearance called freezer burn. It is not really a \u201cburn,\u201d and the food has not necessarily gone bad, although it looks unappetizing. Freezer burn can be minimized by lowering a freezer\u2019s temperature and by wrapping foods tightly so water does not have any space to sublime into.<\/p>\r\nDeposition<\/strong> is the opposite of sublimation in that molecules leave the gas phase and go directly to the solid phase when they hit a cold object.\r\n

      gas \u2192 solid \u00a0 (deposition)<\/strong><\/span><\/span><\/p>\r\nThe formation of frost on a car windshield is an example of deposition, as is the formation of snowflakes in clouds.\u00a0 The lacy appearance of frost and snow flakes reflects their molecule-by-molecule deposition on a cold surface.\u00a0 In contrast, ice looks smooth because a water sample went from liquid to solid in bulk, not molecule-by-molecule.\r\n\r\n<\/div>\r\n<\/div>\r\n

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      Concept Review Exercises<\/h3>\r\n
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        Explain what happens when heat flows into or out of a substance at its melting point or boiling point.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

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        How does the amount of heat required for a phase change relate to the mass of the substance?<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n

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        Answers<\/h3>\r\n[reveal-answer q=\"402994\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"402994\"]\r\n
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        1. The energy goes into changing the phase, not the temperature.<\/li>\r\n \t
        2. The amount of heat is a constant per gram of substance.[\/hidden-answer]<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n
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          Key Takeaway<\/h3>\r\n