The law of definite proportions is sometimes called the law of constant composition. An Example of the Law of Definite Proportions Audio 0:32:02.047142 The decomposition of 18.0 g of water (H2O) results in 16.0 g of oxygen (O2) and 2.0 g of hydrogen (H2) an oxygen-to-hydrogen mass ratio of 8:1. Problem Solving: The Law of Definite Proportions Audio 0:32:39.294000 Two samples of carbon dioxide decompose into their constituent elements. One produces 25.6 g oxygen and 9.60 g carbon, the other 21.6 g oxygen, and 8.10 g carbon. Show that these results are consistent with the law of definite proportions. The Law of Multiple Proportions Audio 0:34:08.719405 In 1804, John Dalton published his law of multiple proportions: When two elements (call them A and B) form two different compounds, the masses of element B that combine with 1 g of element A can be expressed as a ratio of small whole numbers. When an atom of A combines with either one, two, three, or more atoms of B, the following molecular compounds are possible: AB1, AB2, AB3, etc. Audio 0:36:00.257154 Carbon monoxide and carbon dioxide are two compounds composed of the same two elements: carbon and oxygen. The mass ratio of oxygen to carbon in carbon dioxide is 2.67:1; therefore, 2.67 g of oxygen reacts with 1 g of carbon. In carbon monoxide, however, the mass ratio of oxygen to carbon is 1.33:1, or 1.33 g of oxygen to every 1 g of carbon. The ratio of these two masses is itself a small whole number Problem Solving: The Law of Multiple Proportions Nitrogen forms a number of compounds with oxygen. Measurements of the masses of nitrogen and oxygen that form upon decomposing these compounds show that nitrogen dioxide contains 2.28 g oxygen to every 1.00 g of nitrogen, while dinitrogen monoxide contains 0.570 g oxygen to every 1.00 g nitrogen. Show that the results are consistent with the law of multiple proportions:
The law of definite proportions is sometimes called the law of constant composition. An Example of the Law of Definite Proportions Audio 0:32:02.047142 The decomposition of 18.0 g of water (H2O) results in 16.0 g of oxygen (O2) and 2.0 g of hydrogen (H2) an oxygen-to-hydrogen mass ratio of 8:1. Problem Solving: The Law of Definite Proportions Audio 0:32:39.294000 Two samples of carbon dioxide decompose into their constituent elements. One produces 25.6 g oxygen and 9.60 g carbon, the other 21.6 g oxygen, and 8.10 g carbon. Show that these results are consistent with the law of definite proportions. The Law of Multiple Proportions Audio 0:34:08.719405 In 1804, John Dalton published his law of multiple proportions: When two elements (call them A and B) form two different compounds, the masses of element B that combine with 1 g of element A can be expressed as a ratio of small whole numbers. When an atom of A combines with either one, two, three, or more atoms of B, the following molecular compounds are possible: AB1, AB2, AB3, etc. Audio 0:36:00.257154 Carbon monoxide and carbon dioxide are two compounds composed of the same two elements: carbon and oxygen. The mass ratio of oxygen to carbon in carbon dioxide is 2.67:1; therefore, 2.67 g of oxygen reacts with 1 g of carbon. In carbon monoxide, however, the mass ratio of oxygen to carbon is 1.33:1, or 1.33 g of oxygen to every 1 g of carbon. The ratio of these two masses is itself a small whole number Problem Solving: The Law of Multiple Proportions Nitrogen forms a number of compounds with oxygen. Measurements of the masses of nitrogen and oxygen that form upon decomposing these compounds show that nitrogen dioxide contains 2.28 g oxygen to every 1.00 g of nitrogen, while dinitrogen monoxide contains 0.570 g oxygen to every 1.00 g nitrogen. Show that the results are consistent with the law of multiple proportions: