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Law of Conservation of Matter
Law of Conservation of Matter
This law states that "matter cannot be created or destroyed". Atoms cannot appear or disappear into thin air. In chemical reactions they can only be rearranged.
The number of atoms before and after a reaction must be the same.
The mass before and after will weigh the same.
Law of Definite Proportions
Law of Definite Proportions
Chemicals have the same proportions of elements no matter how they are formed.
For example, water,H2O, is composed of 11.19 %H and 88.81% O by mass. All water in the universe will have this compostion.
Another example:
Another example:
Diatomic Gases
Diatomic Gases
Pure elements are said to be in their "elemental form". The chemical formula of most pure elements is simply their elemental symbol. However, some gaseous elements form molecules made of two of the same atoms.
Worksheets
Worksheets
Types of chemical reactions.pdfTypes of Chemical Reactions POGIL (2).pdfbalancing and types practice.docLOADS of Balancing Reactions.doc.docxMole-Mole GPB Wkst.pdfmass-mass GPB Wkst.pdfMass-mass Wkst.docxlimitingReactantsWkst.pdflimitingreagentworksheet.docPercent Yield GPB Wkst.pdfLabs
Labs
Types of Chemical Reactions Lab 18-19.docxAlkaseltzer stoichiometry Lab.pdfGummy Bear Sacrifice.docxClue mystery Lab.docNotes
Notes
11 Types of Chemical Reactions and Balancing.pptxLimiting Reactant Practice Problems.pptxPercent Yield Examples.pptxPage updated
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