. Elementary physics and chemistry: second stage . of temperature of the mercury will be found to be greater than the rise of temperature of the water; in other words, mercury gets hotter than water under the same con- ditions. (Fig. 36.) Blacken two small beakers or flasks of the same size, on the out- side, by holding them in a fish-tail gas burner or over a candle flame. Into one put a convenient mass of water at a known high temperature, and into the other an equal mass of mercury at the same high tempera- ture. Into each insert a thermo- meter. Allow both to cool, and notice that the merc
. Elementary physics and chemistry: second stage . of temperature of the mercury will be found to be greater than the rise of temperature of the water; in other words, mercury gets hotter than water under the same con- ditions. (Fig. 36.) Blacken two small beakers or flasks of the same size, on the out- side, by holding them in a fish-tail gas burner or over a candle flame. Into one put a convenient mass of water at a known high temperature, and into the other an equal mass of mercury at the same high tempera- ture. Into each insert a thermo- meter. Allow both to cool, and notice that the mercury cools much —Equalmassesofwater more rapidly than the water. and mercury do not become hot Different heatins; effects of sub- at equal rates, though they both -^ ^> uj j have the same opportunity. stances at the Same temperature.— Obtain balls of different metals of, say, lead, iron, tin, bismuth, with hooks attached; also a cake of bees-wax about j inch thick, and arrange it on the ring of a retort stand, as in Fig. 38. Then suspend the balls from a wire support (as shown) in a bath of oil heated to about 150° C, and drop them together on to the cake of wax ; notice the iron ball melts through first, then the tin, followed by the lead, and last of all the bismuth. REASONS AND RESULTS. Relative capacity for heat.—So far we have only considered {he amount of heat in water, and you have seen that it depends upon the mass of the water and its temperature. You may think, therefore, that as any mass of water at a certain tempera- ture contains a certain quantity of heat, the same mass of another substance at the same temperature contains the same quantity of heat. This, however, is not the case. A hundred grams of water at a temperature of 50° C. always contain 5000 units of heat, but 100 grams of turpentine, mercury, lead, iron or any other substance at the same temperature as the water, namely 50° C, do not contain this number of units of heat. The quantity o
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