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Topics for each state include: pressure conversions, relationship between Kelvin and kinetic energy, phase changes, intermolecular forces, types of solids, phase diagrams and much more! Finally, because liquids are higher in energy than solids, and lower in energy than gasses the middle slanted line must be the liquid phase. The enthalpy of vaporization gives the amount of energy required to evaporate a liquid at its boiling point, in units of energy per mole. Therefore only the segments that are at an incline will have the substance in just one phase. Which segment represents only the liquid phase? What is the total length of the time that the substance exists only as a liquid? When the kinetic energy is increasing (the temperature is also increasing) the substance is not going through a phase change. Therefore the kinetic energy increases whenever the temperature is increasing. All AP Chemistry Resources.

Phase Change Diagram Answer Key West

The formula becomes: Example Question #4: Energy Of Phase Changes. How much heat must be added to raise a sample of 100g of water at 270K to 280K? Explain your answer. Why does water boil at a lower temperature at high elevation? Is the total length of time it took for the substance to change from liquid to solid? The atmospheric pressure is lower at high elevations. Heat is transferred from the water to the air, resulting in an increase in the temperature of the air.

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The atmospheric pressure is lower at high elevation, so water boils at a lower temperature. What is the melting point of the substance? The total energy requirement to heat a given amount of steam is found by mulitplying the the number of moles to be vaporized by the energy of vaporization per mole. As a substance condenses from the gas phase to the liquid phase, it loses energy in the form of heat loss. Boiling is a phase change from liquids to gas. Increasing temperature means that vapor pressure increases as well. At which segment or segments is the substance exists in two phases? 0 2 4 6 8 10 12 14 16 18 20 22 24 26 28 30 32 34 36 38 40 42 44.

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However, in the event of a phase change (water melts at 273K), the heat of fusion or vaporization must be added to the total energy cost. Is impossible to determine. So, the kinetic energy is increasing during segments 1, 3, and 5. Potential energy of the substance remains constant during which segment or segments? The diagram below shows the cooling of a substance starting with the substance at a temperature above it.

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Is the diagram a heating curve of water or of a different substance? How much energy is required to boil 9 moles of liquid water at its boiling point, and what is the temperature of the water vapor product? The beginning of segment 5. 140 C. Temperature ( o C) 120 D. 80.

Phase Change Diagram Explained

What is the total length of time that the substance undergoes fusion? The specific heat capacity of water is, and water's heat of fusion is. Water has a higher vapor pressure at high elevation. Using the heating curve, determine which segment(s) relate to an increase in potential energy. 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21. In this case it is labeled as segment 3. The following fomula gives the heat needed to generate a given temperature change for a substance of known specific heat capacity: where is the heat input in Joules, is the mass of the sample in grams, and is the specific heat capacity in. The flat areas of the graph represent areas in which heat is being added, but there is no corresponding increase in temperature. Remember, temperature is a measure of the average kinetic energy.

B C. Temperature ( o C) 50. Using the heat curve, define the segment time(s) that the kinetic energy of the substance is increasing. Therefore the substance is boiling during segment 4. At what temperature are the solid and liquid phases exist at equilibrium? What is the phase or phases of the substance during segment C? Therefore we are looking for a segment that is flat (because the potential energy is increasing) and that is between the liquid and gas phases.