1 / 13

Presentation by: Bruce Maples EDU 529 Individual PowerPoint Assignment For Dr. Li 6/30/03

Presentation by: Bruce Maples EDU 529 Individual PowerPoint Assignment For Dr. Li 6/30/03. FIVE BASIC WAYS TO CLASSIFY CHEMICAL REACTIONS:. Synthesis Decomposition Single-Replacement Double-Replacement Combustion. Synthesis Reactions:.

tasha-blackwell
Download Presentation

Presentation by: Bruce Maples EDU 529 Individual PowerPoint Assignment For Dr. Li 6/30/03

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. Presentation by: Bruce Maples EDU 529 Individual PowerPoint Assignment For Dr. Li 6/30/03

  2. FIVE BASIC WAYS TO CLASSIFY CHEMICAL REACTIONS: • Synthesis • Decomposition • Single-Replacement • Double-Replacement • Combustion

  3. Synthesis Reactions: • A synthesis reaction generally follows this equation: • X + Y-->XY • In this equation, X and Y can be compounds or elements. The result XY is a compound.

  4. Examples of Synthesis Reactions: • 2Ba + O2 -->2BaO • 4Cu+ + O2 -->2Cu2O • 2Cu++ + O2 -->2CuO • 2H2 + O2 -->2H2O • C + O2 -->CO2 • 2Na + Cl2 -->2NaCl2

  5. Decomposition Reactions: • In a decomposition reaction, an element or compound is broken down into two simpler substances. The general formula of a decomposition reaction is: • XY --> X + Y • Decomposition reactions are the opposite of synthesis reactions.

  6. Examples of Decomposition Reactions: • 2HgO --> 2Hg + O2 • 2H2O --> 2H2 + O2 • CaCO3 --> CaO + CO2 • Cu(OH)2 --> CuO + H2O • 2KClO3 --> 2KCl + 3O2H2SO4 --> SO3 + H2O

  7. Single Replacement Reactions: • In this type of reaction, one element replaces a similar element in a compound. There are two general equations for single-replacement reactions. They are: • A + XY --> AY + X • A + XY --> XA + Y • In this equation, A, X, and Y are the elements and XY, AY, and XA are the compounds.

  8. Examples of Single Replacement Reactions: • 2Al + 3Fe(NO3)2 --> 3Fe + 2Al(NO3)3 • 2Na + 2H2O --> 2NaOH + H2 • 3Fe + 4H2O --> Fe3O4 + 4H2 • Mg + 2HCl --> MgCl2 + H2 • Cl2 + 2KBr --> 2KCl + Br2

  9. Double-Replacement Reactions: • In a double-replacement reaction, the two compounds exchange places in a solution to form two new compounds. The general equation of a double-replacement reaction is: • AB + XY --> AY + BX

  10. Examples of Double-Replacement Reactions: • Pb(NO3)2 + 2KI --> PbI2 + 2KNO3 • FeS + 2HCl --> H2S + FeCl2 • HCl + NaOH --> NaCl + H2O

  11. Combustion Reactions: • When a substance combines with oxygen releasing a large amount of energy in the form of light and heat, it is a combustion reaction.

  12. Examples of Combustion Reactions: • An example of a combustion reaction is: • C3H8 + 5O2 --> 3CO2 + 4H2O

  13. Presented by Bruce Maples EDU 529 Individual PowerPoint Presentatio For Dr. Sha Li 6/30/03

More Related