Part 34 (1/2)

2. What are two advantages in the expansion of water while freezing?

3. How much heat will be required to melt 1000 g. of ice and warm the water to 20C.?

4. How many grams of ice at 0C. can be melted by 400 g. of water at 55C.?

5. What are two advantages of the high specific heat of water? Two disadvantages?

6. If the specific heat of iron is 0.1125, how much ice at 0C. can be melted by a 200-g. ball of iron heated to 300C?

7. What is the temperature of a hot ball of iron weighing 80 g., if when placed on a piece of ice at 0C. it melts 90 g. of ice?

8. If 500 g. of copper at 400C. are placed into 3000 g. of water at 10C. what will be the resulting temperature?

9. What weight of water at 90C. will just melt 10 kg. of ice at 0C.?

10. If the smooth dry surface of two pieces of ice are pressed together for a short time the two pieces will be frozen into one piece. Explain.

11. Tubs of hot water are sometimes placed in vegetable cellars to prevent the vegetables from freezing. Explain.

12. How many B.t.u. are given out when 2 lbs. of water freeze?

(2) HEAT AND CHANGE OF STATE

[Ill.u.s.tration: FIG. 153.--The black cube in the upper corner represents one cubic inch of water. The entire cube represents the s.p.a.ce occupied by the cubic inch of water in the form of steam. The reduced s.p.a.ces at the bottom and sides show how much short the cube is of being one cubic foot. (American Radiator Co.)]

=184. Heat of Vaporization.=--In our study of evaporation in Art. 174 we considered the more rapidly moving or vibrating molecules in the liquid escaping to the air above and the slower moving molecules being left behind in the liquid; this means that a loss of heat will result upon evaporation, the liquid remaining becoming cooler as the process continues. Now just as a ball thrown up in the air loses its kinetic energy as it rises, and acquires energy of position or potential energy, so molecules escaping from a liquid lose a certain amount of kinetic energy or heat and acquire a corresponding amount of _energy of position_ or potential energy. _Conversely_, as the ball returns to the ground its potential energy is changed to kinetic energy. Similarly when vapor molecules return to the liquid condition they lose their energy of position and acquire kinetic energy. In other words, when a liquid evaporates a certain amount of heat disappears, or becomes _latent_ and when the vapor condenses the heat reappears, or becomes _sensible_ heat.

_The amount of heat that disappears when 1 g. of a substance is vaporized is called the heat of vaporization._ In the case of water at its boiling point, 536 calories of heat disappear when 1 g. of water turns to vapor, and this same amount of heat reappears when the vapor condenses.

The change of volume of water on turning to steam is shown in Fig. 153.

[Ill.u.s.tration: FIG. 154.--Effect of pressure on the boiling point.]

=185. The Boiling Point.=--The boiling temperature depends upon the pressure. The boiling point may be defined as _the temperature at which bubbles of vapor are formed within the liquid_. These bubbles increase the surface at which evaporation can take place in the liquid, and the princ.i.p.al reason why rapid application of heat to a liquid does not raise its temperature above the boiling point is that as more heat is applied more bubbles form so that the increase of evaporating surface supplies a correspondingly greater surface for cooling. The variation of the boiling temperature with changing pressure may be shown by partly filling a strong 7/8-in. test-tube with water. Close the neck with a one-hole rubber stopper through which pa.s.ses a gla.s.s tube to which is attached a soft rubber tube. (See Fig. 154.) Support the tube by a holder, heat the water and boil until all the air is driven from the tube, then close the soft rubber tube with a pinch c.o.c.k and hold the tube in an inverted position. On cooling the end of the tube above the water with cold water or snow, the vapor within is condensed and the pressure upon the water is reduced. Vigorous boiling begins at once. By condensing the vapor repeatedly the water may be made to boil at the room temperature. At the top of Mt. Blanc water boils at 84C. While in steam boilers at 225 lbs. pressure to the square inch the boiling point is nearly 200C.

=186. Laws of Boiling.=--The following statements have been found by experiments to be true.

1. Every liquid has its own _boiling_ point which under the same conditions of _pressure_ is always the same.

2. The temperature of the boiling liquid remains at the boiling point until all the liquid is changed into vapor.

3. The boiling point rises with increased pressure and falls if the pressure is diminished.

4. A boiling liquid and the vapor formed from it have the same temperature. On cooling, a vapor will liquefy at the boiling point.

[Ill.u.s.tration: FIG. 155.--Distilling apparatus.]

5. The solution of solid substances in a liquid raises its boiling point, additional energy being needed to overcome the adhesion involved in the solution. The boiling point is also affected by the character of the vessel containing the liquid. In gla.s.s the boiling point is 101.