Question 1 (Mandatory) (4 points)According to the phase diagram below the solid and liquid phases exist in equilibrium along linePressure (atm)A) ADB) CBC) CDD) AB1.00.7D15.030.0Temperature (°C)45.0How many atoms are contained in a face centered cubic cell? Look at the picture tohelp your reasoningA) There are 14 atomsB) There are 8 corner atoms (only of each atom belongs to the cell) and 4atoms on each of the faces of the cube (only of each atom belongs to thecell). Thus there is a total of 8x+4x=3 atoms.C) There are 8 corner atoms but only of each atom belongs to the cell andthen there are 6 atoms on each face of the cube. There is a total of 8x+6-7 atomsD) There are 8 corner atoms (only 1 over 8 of each atom belongs to the cell)and 6 atoms on each of the faces of the cube (only 1 half of each atombelongs to the cell). Thus there is a total of 8 x 1 over 8+6x1 half = 4atoms.

Option a: This option is correct or incorrect because Option b: This option is correct or incorrect…

Answered: Question 1 (Mandatory) (4 points)…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter9: Liquids And Solids

Section: Chapter Questions

Problem 21QAP: Given the following data about xenon,...

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8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?
Silicon carbide, SiC, is a very hard, high-melting solid. What kind of crystal forces account for these properties?
If you've ever opened a bottle of rubbing alcohol or other solvent on a warm day, you may have heard a little “whoosh” as the vapor that had built up above the liquid escapes. Describe on a microscopic basis how a vapor pressure builds up in a closed container above a liquid. What processes in the container give rise to this phenomenon?
Referring to Figure 9.7, state what phase(s) is/are present at (a) 1 atm, 100C. (b) 0.5 atm, 100C.(c) 0.8 atm. 50C.
The vapor pressure of I2(s) at 30C is 0.466 mm Hg. (a) How many milligrams of iodine will sublime into an evacuated 750.0-mL flask? (b) If 3.00 mg of I2 are used, what will the final pressure in the flask be? (c) If 7.85 mg of I2 are used, what will the final pressure in the flask be?
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.
8.87 Use the vapor pressure curves illustrated here to answer the questions that follow. (a) What is the vapor pressure of ethanol (C2H5OH) at 60°C? (b) Considering only carbon disulfide (CS2) and ethanol, which has the stranger intermolecular forces in the liquid state? (c) At what temperature does heptane (C7H16) have a vapor pressure of 500 mm Hg? (d) What are the approximate normal boiling pains of each of the three substances? (e) At a pressure of 400 mm Hg and a temperature of 70°C, is each substance a liquid, a gas, or a mixture of liquid and gas?
Describe the behavior of a liquid and its vapor in a closed vessel as the temperature increases.
Consider 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?
The normal boiling point of SO2 is 263.1 K and that of NH3 is 239.7 K. At −40 °C, would you predict that ammonia has a vapor pressure greater than, less than, or equal to that of sulfur dioxide? Explain.
Explain why the molar enthalpies of vaporization of the following substances increase in the order CH4C2H6C3H8, even though the type of IMF (dispersion) is the same.
A common prank on college campuses is to switch the salt and sugar on dining hall tables, which is usually easy because the substances look so much alike. Yet, despite the similarity in their appearance, these two substances differ greatly in their properties, since one is a molecular solid and the other is an ionic solid. How do the properties differ and why?

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