Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution freezing point boiling point 7.7 g of hydroiodic acid (HI) dissolved in 500. mL of water (choose one) 0 (choose one) e 7.7 g of potassium hydroxide (KOH) dissolved in 500. mL of water (choose one) e (choose one) e 7.7 g of calcium chloride (CaCl2) dissolved in 500. mL of water (choose one) e (choose one) 0 500. mL of pure water (choose one) e (choose one) 0

The molecular mass of butanol, C4H9OH, is 74.14; that of ethylene glycol, CH2(OH)CH2OH, is 62.08, yet their boiling points are 117.2 C and 174 C, respectively. Explain the reason for the difference.

In the northern United States, summer cottages are usually closed up for the winter. When doing so, the owners winterize the plumbing by putting antifreeze in the toilet tanks, for example. Will adding 525 g of HOCH2CH2OH to 3.00 kg of water ensure that the water will not freeze at 25 C?

You add 0.255 g of an orange, crystalline compound whose empirical formula is C10H8Fe to 11.12 g of benzene. The boiling point of the benzene rises from 80.10 C to 80.26 C. What are the molar mass and molecular formula of the compound?

Two molecules that contain the same number of each kind of atom but [hat have different molecular structures are said to he isomers of each other. For example, both ethyl alcohol and dimethyl ether (shown below} have the formula C2H6Oand are isomers; Based on considerations of intermolecular forces. which substance would you expect to be more volatile? Which would you expect 10have the higher boiling point? Explain. methyl ether hyl alcohol msp;CH3OCH3CH3CH2OH

5-86 Using the phase diagram of water (Figure 5-20), describe the process by which you can sublime 1 g of ice at-10°C and at 1 atm pressure to water vapor at the same temperature.

Explain why evaporation leads to cooling of the liquid.

How many grams of water at 0C will be melted by the condensation of 1 g of steam at 100C?

Of the four general types of solids, which one(s) (a) are generally low-boiling? (b) are ductile and malleable? (c) are generally soluble in nonpolar solvents?

It is possible to balance a paper clip on the surface of water in a beaker. lf you add a bit of soap to the water, however, the paper clip sinks. Explain how the paper clip can float and why it sinks when soap is added.