File:A popular chemistry; (1887) (14592800828).jpg

English:
Preparing CO2: For experimental purposes, CO2 is prepared by pouring hydrochloric (muriatic) acid on marble or chalk. The CO2 is liberated rapidly, and, as it is much heavier than air, may be collected by downward displacement, while the calcium chloride remains dissolved in the water of the flask

Identifier: popularchemist00stee (find matches)
Title: A popular chemistry;
Year: 1887 (1880s)
Authors: Steele, J(oel) Dorman, 1836-1886. (from old catalog)
Subjects: Chemistry
Publisher: New York and Chicago, A. S. Barnes & company
Contributing Library: The Library of Congress
Digitizing Sponsor: The Library of Congress

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Text Appearing Before Image:
ature inimmense quantities. Wherever C burns, in fires,lights, decay, volcanoes—in a word, in all those va-rious forms of combustion of which we spoke underthe subject of 0, where that gas unites with C, C02is the result. Each adult exhales daily about 8f oz.of carbon changed to this invisible gas. Each bushelof charcoal, in burning, produces not far from 2500gallons. A lighted candle gives off about four gal-lons per hour. Preparation. — For experimental purposes, C02 isprepared by pouring hydrochloric (muriatic) acid onmarble or chalk. The reaction may be representedas follows: CaC03 + 2HC1 = CaCl2 + H20 + C02. The CO2 is liberated rapidly and, as it is muchheavier than air, may be collected by downward dis-placement (see Fig. 25), while the calcium chlorideremains dissolved in the water of the flask. 64: INORGANIC CHEMISTRY. The test for C02 is clear lime-water. If we ex-pose a saucer of lime-water to the air, the surfaceof the solution will soon be covered with a thin Pig. 25.
Text Appearing After Image:
Preparing C02.* film of calcium carbonate (carbonate of lime), thusshowing that there is C02 in the atmosphere; orif we breathe by means of a tube through lime-water, the solution will become turbid and milky,thus proving the presence of C02 in our breath ; bybreathing through the liquid a little longer it willbecome clear, as the carbonate will dissolve in anexcess of C02.f * Twist a wire around the neck of a small, wide-mouthed vial, to serveas a bucket. Dip the C02 with it upward from the jar and test with alighted match. Dip the H (Fig. 15) downward, and test in same way. Thisillustrates in a striking manner the difference between the gases in respectto specific gravity and combustion. t Burn a piece of charcoal or a candle in a jar of O. Pour in a littlelime-water and shake it well, when there will be a precipitation of chalk(calcium carbonate). Hold a jar of air over a burning lamp or jet of coal-gas, or breathe into the jar and apply the test, CARBON. Properties.— CO2 is a co

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