Laws of Definite Proportions & Multiple Proportions

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Presentation transcript:

Laws of Definite Proportions & Multiple Proportions PreAP Chemistry

Law of Definite Proportion Put forth by Joesph Louis Proust (1754-1816) in 1800 States that different samples of the same compound always contain its constituent elements in the same proportion by mass regardless of the source. It is an intensive property. Example CO and CO2 CO = O/C = 1/1 CO2 = O/C =2/1 CO to CO2 = 1:2

Calculation Mass Fraction = Mass of element Mass of Compound Mass Percent = Mass of element x 100 Mass of element in a sample = Mass of compound x Mass of element in a sample Mass of Compound

Law of Multiple Proportions Derived by John Dalton (1766-1844) in between 1803-1807. States if two elements A and B combine to form more than one compound, the masses of B that can combine with a given mass of A are in a ratio of small whole numbers. It is an intensive property. Example – H2O and H2O2

Ratio of O mass with a constant mass of Sn Example Compound Mass of Tin (Sn) in g Mass of Oxygen (O) in g Ratio of O mass with a constant mass of Sn Tin (II) Oxide SnO 119 g 16 g 1 Tin (IV) Oxide SnO2 32 g 2

Difference between Laws of multiple proportions and definite proportions Both laws have to do with relating to Dalton's Atomic Theory. The only difference is that the Law of Definite Proportions deals with elements combining to form ONE compound in a simple whole number ratio. The Law of Multiple Proportions is comparing the same 2 elements that make up 2 different compounds, the division of these 2 ratios should equal a simple whole number ratio. For example: Carbon and oxygen can combine to form carbon monoxide and carbon dioxide. If you calculated each compounds ration of oxygen to carbon you would get the following ratios: compound A would equal a combining ratio of 1.34:1 (O:C). Compound B would equal a combining ratio of 2.67:1 (O:C). If you divided the bigger ratio by the smaller ratio you would have that oxygen combines with a ratio of 2.67/1.34 which would equal 1.99:1, which is close enough to 2:1.