(a)
Interpretation:
The given true and false statements of given phase diagram are should be identified.
Concept Introduction:
Phase diagram:
The plot of temperature against pressure is called phase diagram. It contains the information of boiling and melting points and critical temperature and pressure of the substance.
(b)
Interpretation:
The given true and false statements of given phase diagram are should be identified.
Concept Introduction:
Phase diagram:
The plot of temperature against pressure is called phase diagram. It contains the information of boiling and melting points and critical temperature and pressure of the substance.
(c)
Interpretation:
The given true and false statements of given phase diagram are should be identified.
Concept Introduction:
Phase diagram:
The plot of temperature against pressure is called phase diagram. It contains the information of boiling and melting points and critical temperature and pressure of the substance.
(d)
Interpretation:
The given true and false statements of given phase diagram are should be identified.
Concept Introduction:
Phase diagram:
The plot of temperature against pressure is called phase diagram. It contains the information of boiling and melting points and critical temperature and pressure of the substance.
(e)
Interpretation:
The given true and false statements of given phase diagram are should be identified.
Concept Introduction:
Phase diagram:
The plot of temperature against pressure is called phase diagram. It contains the information of boiling and melting points and critical temperature and pressure of the substance.
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Chapter 9 Solutions
Chemistry: An Atoms First Approach
- A 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_forwardElemental carbon has one gas phase, one liquid phase, and two different solid phases, as shown in the phase diagram: (a) On the phase diagram, label the gas and liquid regions. (b) Graphite is the most stable phase of carbon at normal conditions. On the phase diagram, label the graphite phase. (c) If graphite at normal conditions is heated to 2500 K while the pressure is increased to 1010 Pa, it is converted into diamond. Label the diamond phase. (d) Circle each triple point on the phase diagram. (e) In what phase does carbon exist at 5000 K and 108 Pa? (f) If the temperature of a sample of carbon increases from 3000 K to 5000 K at a constant pressure of 106 Pa, which phase transition occurs, if any?arrow_forwardDry ice, CO2(s) , does not melt at atmospheric pressure. It sublimes at a temperature of 78 °C. What is the lowest pressure at which CO2(s) will melt to give CO2(l) ? At approximately what temperature will this occur? (See Figure 10.34 for the phase diagram.)arrow_forward
- The 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_forwardPhase diagrams for materials that have allotropes can be more complicated than those shown in the chapter. Use the phase diagram for carbon given here to answer the following questions. (a) How many triple points are present and what phases are in equilibrium for each? (b) Is there a single point where all four phases are in equilibrium? (c) Which is more stable at high pressures, diamond or graphite? (d) Which is the stable phase of carbon at room temperature and 1 atmosphere pressure?arrow_forward
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