11.8 At three different temperatures, Ti, T, and T, the molecules in a liquid crystal align in these ways: 2.1 5EL6 Тз T2 T1 (a) At which temperature or temperatures is the substance in a liquid crystalline state? At those temperatures, which type of liquid crystalline phase is depicted? (b) Which is the highest of these three temperatures? [Section 11.7)

11.8 At three different temperatures, Ti, T, and T, the molecules in a liquid crystal align in these ways: 2.1 5EL6 Тз T2 T1 (a) At which temperature or temperatures is the substance in a liquid crystalline state? At those temperatures, which type of liquid crystalline phase is depicted? (b) Which is the highest of these three temperatures? [Section 11.7)

Chemistry by OpenStax (2015-05-04)

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ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter10: Liquids And Solids

Section: Chapter Questions

Problem 8E: The types of intermolecular forces in a substance are identical whether it is a solid, a liquid, or...

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Similar questions

Referring 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.
8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?
The types of intermolecular forces in a substance are identical whether it is a solid, a liquid, or a gas. Why then does a substance change phase from a gas to a liquid or to a solid?
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 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.
The vapor pressure of ethanol, C2H5OH, at 50.0 C is 233 mmHg, and its normal boiling point at 1 atm is 78.3 C. Calculate the vapH of ethanol.
Silicon carbide, SiC, is a very hard, high-melting solid. What kind of crystal forces account for these properties?
At three different temperatures, T1, T2, and T3, the moleculesin a liquid crystal align in these ways: (a) At which temperature or temperatures is the substancein a liquid crystalline state? At those temperatures, whichtype of liquid crystalline phase is depicted? (b) Which is thehighest of these three temperatures?
At three different temperatures, T1, T2, and T3, the moleculesin a liquid crystal align in these ways:T1(a) At which temperature or temperatures is the substancein a liquid crystalline state? At those temperatures, whichtype of liquid crystalline phase is depicted? (b) Which is thehighest of these three temperatures? [Section 11.7]
Hydrogen peroxide (H2O2) is a major industrial chemicalthat is produced on a scale approaching 109 kg per year. Itis widely used as a bleach and in chemical manufacturingprocesses. How do you expect its boiling point to comparewith those of fluorine (F2) and hydrogen sulfide (H2S), twosubstances with molar masses comparable with that ofhydrogen peroxide?
The moleculeshave the same molecular formula 1C3H8O2 but differentchemical structures. (a) Which molecule(s), if any, canengage in hydrogen bonding? (b) Which molecule do youexpect to have a larger dipole moment? (c) One of these moleculeshas a normal boiling point of 97.2 °C, while the otherone has a normal boiling point of 10.8 °C. Assign each moleculeto its normal boiling point. [Sections 11.2 and 11.5]
Explain why the molar enthalpies of vaporization of the following substances increase in the order CH4 < C2H6 < C3H8, even though the type of IMF (dispersion) is the same.

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