Law of Definite Composition and Law of Multiple Proportions Chemistry Mrs. Coyle

Joseph Proust (France 1799) Law of Definite Proportions: A given compound always contains elements in a certain proportion by mass. (Constant composition).

Atoms combine in whole number ratios, so their proportion by mass will always be the same. Example: H2O is always made up of 2 atoms of H and one atom of O. The ratio of O to H in water is always 16:2 or 8:1.

Example: KCl always contains one atom of K for every one atom of Cl In KCl, potassium and chlorine always have a ratio of “39.09 to 35.45” or “1.1 to 1” by mass.

Law of Multiple Proportions (John Dalton) When two elements combine to form more than one compound, the ratios of the mass of one element in the first compound to its mass in the second compound, (as it combines with the same mass of the other element), can always be expressed as ratios of small whole numbers( ex: 1:3 or 2:5).

Example of Law of Multiple Proportions Carbon combines with oxygen to form CO and CO2 . Mass of Carbon(g) Mass of Oxygen(g) Ratio of O in CO2 to O in CO CO 12.01 16.00 CO2 32.00 2:1

Practice Problem 1 In the carbon compounds ethane (C2H6) and ethene (C2H4), what is the lowest whole number ratio of H atoms that react with the same number of C atoms?

Practice Problem 2 Carbon reacts with oxygen to form two compounds. Compound A contains 2.41 g of carbon for each 3.22 g of oxygen. Compound B contains 6.71 g of carbon for each 17.9 g of oxygen.

Solution Strategy Find the grams of carbon per 1 g of oxygen for each compound. Divide the highest answer by the smallest answer.

Answer 2:1

Practice Problem 3 Lead forms two compounds with oxygen. One contains 2.98 g of lead and 0.461 g of oxygen. The other contains 9.89 g of lead and 0.763 g of oxygen. For a given mass of oxygen, what is the lowest whole number mass ratio of lead in the two compounds? Answer: 2:1