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373 Temperature (K)

273 243 A

8137 Heat (J)

Table 12-2

Heats of Fusion and Vaporization of Common Substances Material Copper Mercury Gold Methanol Iron Silver Lead Water (ice) Heat of Fusion Hf (J/kg) 205 115 630 109 266 104 204 334 105 104 104 105 105 105 104 105 Heat of Vaporization Hv (J/kg) 507 272 164 878 629 236 864 226 106 105 106 105 106 106 105 106

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As in melting, the temperature does not rise while a liquid boils In Figure 12-10, this transition is represented between points D and E After the material is entirely converted to gas, any added thermal energy again increases the motion of the particles, and the temperature rises Above point E, steam is heated to temperatures greater than 373 K

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Heat of fusion The amount of energy needed to melt 1 kg of a substance is called the heat of fusion of that substance For example, the heat of fusion of ice is 334 105 J/kg If 1 kg of ice at its melting point, 273 K, absorbs 334 105 J, the ice becomes 1 kg of water at the same temperature, 273 K The added energy causes a change in state but not in temperature The horizontal distance in Figure 12-10 from point B to point C represents the heat of fusion Heat of vaporization At normal atmospheric pressure, water boils at 373 K The thermal energy needed to vaporize 1 kg of a liquid is called the heat of vaporization For water, the heat of vaporization is 226 106 J/kg The distance from point D to point E in Figure 12-10 represents the heat of vaporization Every material has a characteristic heat of vaporization Between points A and B, there is a definite slope to the line as the temperature is raised This slope represents the specific heat of the ice The slope between points C and D represents the specific heat of water, and the slope above point E represents the specific heat of steam Note that the slope for water is less than those of both ice and steam This is because water has a greater specific heat than does ice or steam The heat, Q, required to melt a solid of mass m is given by the following equation Heat Required to Melt a Solid Q mHf

1 Label two foam cups A and B 2 Measure and pour 75 mL of room-temperature water into each cup Wipe up any spilled liquid 3 Add an ice cube to cup A, and add ice water to cup B until the water levels are equal 4 Measure the temperature of the water in each cup at 1-min intervals until the ice has melted 5 Record the temperatures in a data table and plot a graph Analyze and Conclude 6 Do the samples reach the same final temperature Why

The heat required to melt a solid is equal to the mass of the solid times the heat of fusion of the solid

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