(a)
Interpretation:
The position of solid, liquid and vapor in phase diagram should be determined.
Concept introduction:
Phase diagram is a graph that represents the solid phase, liquid phase, and gaseous phase of one substance or mixture of substance under different states of temperature and pressure.
The temperature and pressure on a phase diagram at which gas, liquid, and solid phases coexist is called triple point. The temperature and pressure in the phase diagram at which substance is lies between liquid-gas phases is called critical point. The temperature and pressure at which liquid or gas is neither a true liquid nor a true gas is called supercritical point.
(b)
Interpretation:
The number of triple point of carbon should be determined. Also, the triple point in phase diagram should be circled.
Concept introduction:
Phase diagram is a graph that represents the solid phase, liquid phase, and gaseous phase of one substance or mixture of substance under different states of temperature and pressure.
The temperature and pressure in the phase diagram at which substance is lies between liquid-gas phases is called critical point. The temperature and pressure at which liquid or gas is neither a true liquid nor a true gas is called supercritical point.
(c)
Interpretation:
The graphite phase on the diagram should be identified.
Concept introduction:
Phase diagram is a graph that represents the solid phase, liquid phase, and gaseous phase of one substance or mixture of substance under different states of temperature and pressure.
The temperature and pressure in the phase diagram at which substance is lies between liquid-gas phases is called critical point. The temperature and pressure at which liquid or gas is neither a true liquid nor a true gas is called supercritical point.
d)
Interpretation:
The diamond phase on the diagram is to be identified.
Concept introduction:
Phase diagram is a graph that represents the solid phase, liquid phase, and gaseous phase of one substance or mixture of substance under different states of temperature and pressure.
The temperature and pressure in the phase diagram at which substance is lies between liquid-gas phases is called critical point. The temperature and pressure at which liquid or gas is neither a true liquid nor a true gas is called supercritical point.
(e)
Interpretation:
Whether the graphite or diamond phase that is more denser should be determined.
Concept introduction:
Phase diagram is a graph that represents the solid phase, liquid phase, and gaseous phase of one substance or mixture of substance under different states of temperature and pressure.
The temperature and pressure in the phase diagram at which substance is lies between liquid-gas phases is called critical point. The temperature and pressure at which liquid or gas is neither a true liquid nor a true gas is called supercritical point.
The density of phase is determined by temperature and pressure of the phase in the phase diagram. The phase that lies in high pressure and low temperature range is more dense.
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Chapter 11 Solutions
CHEMISTRY-TEXT
- Use the phase diagram for sulfur for Question 75. The solid forms of sulfur are rhombic and monoclinic. (a) A triple point is defined as a temperature and pressure where three phases are in equilibrium. How many triple points does sulfur have? Indicate the approximate temperature and pressure at each. (b) Which physical states are present at equilibrium under these conditions? (i) 102 atm and 80 C (ii) 101 atm and 140 C (iii) 103 atm and 110 C (iv) 104 atm and 160 C Phase diagram for sulfur, for Question 75.arrow_forwardA special vessel (see Fig. 10.45) contains ice and supercooled water (both at 10C) connected by vapor space. Describe what happens to the amounts of ice and water as time passes.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
- On the basis of the description given, classify each of these solids as molecular, metallic, ionic, network, or amorphous, and explain your reasoning. (a) A brittle, yellow solid that melts at 113 C; neither the solid nor the liquid conducts electricity (b) A soft, silvery solid that melts at 40 C; both the solid and the liquid conduct electricity (c) A hard, colorless, crystalline solid that melts at 1713 C; neither the solid nor the liquid conducts electricity (d) A soft, slippery solid that melts at 63 C; neither the solid nor the liquid conducts electricityarrow_forwardThe amount of heat required to melt 2 lbs of ice is twice the amount of heat required to melt 1 lb of ice. Is this observation a macroscopic or microscopic description of chemical behavior? Explain your answer.arrow_forwardThe enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.arrow_forward
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