1 / 9

Definite Proportions, Multiple Proportions and Atomic Theory

Definite Proportions, Multiple Proportions and Atomic Theory. The sum of the masses for the reactants equals the sum of the masses for the products. Law of Conservation of Mass. Lavoisier Mass is neither created nor destroyed in a chemical reaction

fishera
Télécharger la présentation

Definite Proportions, Multiple Proportions and Atomic Theory

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Definite Proportions, Multiple Proportions and Atomic Theory

  2. The sum of the masses for the reactants equals the sum of the masses for the products Law of Conservation of Mass • Lavoisier • Mass is neither created nor destroyed in a chemical reaction • If you start with 10g, you will wind up with 10g

  3. Law of Definite Proportions • Proust • Atoms are neither lost nor gained in a chemical reaction • Chemical compounds have the same mass ratio of elements no matter how formed (e.g., water always has an O to H ratio of 8.01:1.00) • Evidence for this law: Berzelius’ experiments with lead and sulfur • Constant composition implies constant properties (i.e., water always boils at 100ºC and freezes at 0ºC)

  4. Chemical compounds have the same mass ratio of elements no matter how formed Copper Carbonate

  5. Law of Definite Proportions

  6. Law of Multiple Proportions • Compounds of differing mass ratios of the same elements are found, but they will have different properties • Example: carbon dioxide (CO2) and carbon monoxide (CO)

  7. Dalton’s Atomic Theory • John Dalton- (1803) Law of Multiple Proportions, Atomic Theory of Matter • Elements of Dalton’s atomic theory: • Matter is composed of atoms • Different elements have different atoms • (e.g, C has a mass=12, O has a mass=16) • Compounds form when different elements combine in fixed proportions

  8. Determining the Mass of a Compound • EXAMPLE: • If C has a mass of 12 and O has a mass of 16, what is the mass of: • a) Carbon monoxide (CO) • 12 + 16 = 28 • b) Carbon dioxide (CO2) • 12 + 2(16) = 44

  9. Determining the Mass of a Compound • Find the mass of NaCl, NaOH, CaCO3, and H2SO4 • The atomic masses for each element are found on the periodic table. (for now use these amounts) Na=23 Cl=35 O=16 Ca=40 C=12 H=1 and S=32

More Related