Chapter 11: Problem 70
Describe how a cholesteric liquid crystalline phase differs from a smectic A liquid crystalline phase.
Chapter 11: Problem 70
Describe how a cholesteric liquid crystalline phase differs from a smectic A liquid crystalline phase.
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Get started for freeName the phase transition in each of the following situations and indicate whether it is exothermic or endothermic: (a) Iodine solid turns to iodine gas when it is heated. (b) Snowflakes turn into water when they fall on an open palm. (c) Droplets of water appear on grass in a cold humid morning. (d) Dry ice gradually disappears when left at room temperature for some period of time.
Propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) is pressurized into liquid and stored in cylinders to be used as a fuel. The normal boiling point of propane is listed as \(-42^{\circ} \mathrm{C}\). (a) When converting propane into liquid at room temperature of \(25^{\circ} \mathrm{C},\) would you expect the pressure in the tank to be greater or less than atmospheric pressure? How does the pressure within the tank depend on how much liquid propane is in it? (b) Suppose the fuel tank leaks and a few liters of propane escape rapidly. What do you expect would happen to the temperature of the remaining liquid propane in the tank? Explain. (c) How much heat must be added to vaporize $20 \mathrm{~g}\( of propane if its heat of vaporization is \)18.8 \mathrm{~kJ} / \mathrm{mol} ?\( What volume does this amount of propane occupy at \)100 \mathrm{kPa}\( and \)25^{\circ} \mathrm{C} ?$
(a) Place the following substances in order of increasing volatility: $\mathrm{CH}_{4}, \mathrm{CBr}_{4}, \mathrm{CH}_{2} \mathrm{Cl}_{2}, \mathrm{CH}_{3} \mathrm{Cl}, \mathrm{CHBr}_{3},\( and \)\mathrm{CH}_{2} \mathrm{Br}_{2}$. (b) How do the boiling points vary through this series? (c) Explain your answer to part (b) in terms of intermolecular forces.
Acetone \(\mathrm{CH}_{3} \mathrm{COCH}_{3}\), is a common organic solvent with relatively low melting point \((178 \mathrm{~K})\) and boiling point $(329 \mathrm{~K})\(. The enthalpy of fusion of acetone is \)5.72 \mathrm{~kJ} / \mathrm{mol}\(, and its enthalpy of vaporization is \)29.1 \mathrm{~kJ} / \mathrm{mol}\(. The specific heats of solid and liquid acetone are \)96 \mathrm{~J} / \mathrm{mol}-\mathrm{K}\( and \)125.5 \mathrm{~J} / \mathrm{mol}-\mathrm{K}$ respectively. (a) How much heat is required to convert \(23.0 \mathrm{~g}\) of acetone at \(273 \mathrm{~K}\) to the vapor phase at \(329 \mathrm{~K} ?(\mathbf{b})\) How much heat is required to convert the same amount of acetone at \(77 \mathrm{~K}\) to the vapor phase at $329 \mathrm{~K} ?$
The following data present the temperatures at which certain vapor pressures are achieved for dichloromethane $\left(\mathrm{CH}_{2} \mathrm{Cl}_{2}\right)\( and methyl iodide \)\left(\mathrm{CH}_{3} \mathrm{I}\right):$ (a) Which of the two substances is expected to have the greater dipole-dipole forces? Which is expected to have the greater dispersion forces? Based on your answers, explain why it is difficult to predict which compound would be more volatile. (b) Which compound would you expect to have the higher boiling point? Check your answer in a reference book such as the CRC Handbook of Chemistry and Physics. (c) The order of volatility of these two substances changes as the temperature is increased. What quantity must be different for the two substances for this phenomenon to occur? (d) Substantiate your answer for part (c) by drawing an appropriate graph.
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