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(a)
Interpretation: The number of triple points in the given phase diagram of carbon needs to be determined.
Concept Introduction:
The conversion of
The heating -cooling curve is the curve of temperature v/s time that interpret the change in the states of matter with increase in temperature.
Freezing point is the temperature at which the solid state converts to liquid state or vice-versa. Boiling point is the temperature at which the liquid and gas state reach to an equilibrium hence after this temperature, both states must be in equilibrium.
(b)
Interpretation: The phases which coexist at the triple points in the given phase diagram of carbon needs to be determined.
Concept Introduction:
The conversion of solid to liquid and gas involves the change in temperature that can display in heat curve.
The heating -cooling curve is the curve of temperature v/s time that interpret the change in the states of matter with increase in temperature.
Freezing point is the temperature at which the solid state converts to liquid state or vice-versa. Boiling point is the temperature at which the liquid and gas state reach to an equilibrium hence after this temperature, both states must be in equilibrium.
(c)
Interpretation: The change when graphite is subjected at very high pressure at room temperature needs to be explained.
Concept Introduction:
The conversion of solid to liquid and gas involves the change in temperature that can display in heat curve.
The heating -cooling curve is the curve of temperature v/s time that interpret the change in the states of matter with increase in temperature.
Freezing point is the temperature at which the solid state converts to liquid state or vice-versa. Boiling point is the temperature at which the liquid and gas state reach to an equilibrium hence after this temperature, both states must be in equilibrium.
(d)
Interpretation: The denser state out of graphite and diamond needs to be determined, if the density increases with increasing the pressure.
Concept Introduction:
The conversion of solid to liquid and gas involves the change in temperature that can display in heat curve.
The heating -cooling curve is the curve of temperature v/s time that interpret the change in the states of matter with increase in temperature.
Freezing point is the temperature at which the solid state converts to liquid state or vice-versa. Boiling point is the temperature at which the liquid and gas state reach to an equilibrium hence after this temperature, both states must be in equilibrium.
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Chapter 16 Solutions
Chemical Principles
- 8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?arrow_forwardConsider the following data for xenon: Triple point: 121C, 280 torr Normal melting point: 112C Normal boiling point: 107C Which is more dense, Xe(s) or Xe(l)? How do the melting point and boiling point of xenon depend on pressure?arrow_forwardA pure substance X has the following properties: Mp=90C, increasing slightly as pressure increases; normal bp=120C; liquid vp=65mm Hg at 100C, 20 mm Hg at the triple point. (a) Draw a phase diagram for X. (b) Label solid, liquid, and vapor regions of the diagram. (c) What changes occur if, at a constant pressure of 100 mm Hg, the temperature is raised from 100C to 150C?arrow_forward
- What feature characterizes the dynamic equilibrium between a liquid and its vapor in a closed container?arrow_forwardSilicon carbide, SiC, is a very hard, high-melting solid. What kind of crystal forces account for these properties?arrow_forwardRubidium chloride has the sodium chloride structure at normal pressures but assumes the cesium chloride structure at high pressures. (See Exercise 69.) What ratio of densities is expected for these two forms? Does this change in structure make sense on the basis of simple models? The ionic radius is 148 pm for Rb+ and 181 pm for CI.arrow_forward
- An amorphous solid can sometimes be converted to a crystalline solid by a process called annealing. Annealing consists of heating the substance to a temperature just below the melting point of the crystalline form and then cooling it slowly. Explain why this process helps produce a crystalline solid.arrow_forwardReferring to Figure 9.7, state what phase(s) is (are) present at (a) 1 atm, 10C. (b) 3 mm Hg, 20C. (c) 1000 mm Hg, 75C.arrow_forwardThe phase diagram for water over a relative narrow pressure and temperature range is given in Figure 9.19. A phase diagram over a considerably wider range of temperature and pressure (kbar) is given nearby. This phase diagram illustrates the polymorphism of ice, the existence of a solid in more than one form. In this case, Roman numerals are used to designate each polymorphic form. For example, Ice I, ordinary ice, is the form that exists under ordinary pressures. The other forms exist only at higher pressures, in some cases extremely high pressure such as Ice VII and Ice VIII. Using the phase diagram, give the approximate P and T conditions at the triple point for Ice III, Ice V, and liquid water. Determine the approximate temperature and pressure for the triple point for Ices VI, VII, and VIII. What is anomalously different about the fusion curves for Ice VI and Ice VII compared to that of Ice I? What phases exist at 8 kbar and 20 °C? At a constant temperature of −10 °C, start at 3 kbar and increase the pressure to 7 kbar. Identify all the phase changes that occur sequentially as these conditions change. Explain why there is no triple point for the combination of Ice VII, Ice VIII, and liquid water.arrow_forward
- 8.45 Describe how interactions between molecules affect the vapor pressure of a liquid.arrow_forwardDescribe the behavior of a liquid and its vapor in a closed vessel as the temperature increases.arrow_forwardKrypton, Kr, has a triple point at 169C and 133 mmHg and a critical point at 63C and 54 atm. The density of the solid is 2.8 g/cm3, and the density of the liquid is 2.4 g/cm3. Sketch a rough phase diagram of krypton. Circle the correct word in each of the following sentences (and explain your answers). a Solid krypton at 130 mmHg (melts, sublimes without melting) when the temperature is raised. b Solid krypton at 760 mmHg (melts, sublimes without melting) when the temperature is raised.arrow_forward
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