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Exploring Chemical Reactions: Laws and Processes

Understand chemical reactions with reactants and products, laws of mass and energy conservation, synthesis, decomposition, combustion, replacement reactions, exothermic and endothermic reactions. Explore the world of chemistry!

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Exploring Chemical Reactions: Laws and Processes

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  1. A scientific artifact By bluegreen_fire

  2. What is a chemical reaction? • It’s a process that always results in the combination of the chemical substances involved. • The substance or substances initially involved are called reactants. • The result of a chemical reaction is called the product. http://en.wikipedia.org/wiki/Chemical_reaction

  3. What is the law of mass conservation? • It says the mass of an object will remain constant, no matter what’s going on inside. • Or that mass and or matter cannot be created or destroyed. http://en.wikipedia.org/wiki/Conservation_of_mass

  4. What is the law of energy conservation? • The total amount of energy in an isolated system remains constant. • Energy cannot be created or destroyed. http://en.wikipedia.org/wiki/Conservation_of_energy

  5. What is synthesis? • It’s a series of chemical reactions in order to get a product or several products. • It occurs from physical and chemical changes usually involving one or more reactions. • H2 +O2 H2O http://en.wikipedia.org/wiki/Chemical_synthesis

  6. What is decomposition? • It is basically the opposite of synthesis, because instead of two or more chemicals coming together, they are breaking apart into their original elements. • H2O H2 + O2 • http://en.wikipedia.org/wiki/Chemical_decomposition

  7. What is combustion? • It’s a complex exothermic chemical reaction between a fuel and an oxidant. • The result of this is heat or both heat and light in the form of either a glow or flames. • This is an example of the combustion between hydrogen and oxygen • 2 H2 + O2 2 H2O(g) heat http://en.wikipedia.org/wiki/Combustion

  8. What is single replacement? • It’s a reaction that occurs when two different cations switch places to combine with the same anion. • The link below has a video example of single replacement. • Zn + 2HCl ZnCl2 +H2 http://web.fccj.org/~smilczan/Two5/DR.html

  9. What is double replacement? • It occurs when two ionic compounds are mixed together. • In water the compounds split apart into their respective anions and cations • Now the cations have the opportunity to swap anions. • HCl(aq) + NaOH (aq) NaCl + H2O(l) • http://en.wikipedia.org/wiki/Double_replacement

  10. What are exothermic and endothermic reactions? • An exothermic reaction releases energy in the form of heat, light, or sound. • A good example is fireworks. • C3H +5 O2 3 CO2 +4 H2O http://www.science.uwaterloo.ca/~cchieh/cact/c120/reaction.html • An endothermic reaction must absorb energy to work. • Like when you combine urea and water, the two parts of an ice pack. • 3 H2 + N2 2 NH2 http://www.citycollegiate.com/chapter2a.htm

  11. THE END!!!!!!! =]

  12. Bibliography!!! • http://en.wikipedia.org/wiki/Chemical_reaction • http://en.wikipedia.org/wiki/Conservation_of_mass • http://en.wikipedia.org/wiki/Conservation_of_energy • http://en.wikipedia.org/wiki/Chemical_synthesis • http://en.wikipedia.org/wiki/Chemical_decomposition • http://en.wikipedia.org/wiki/Combustion • http://web.fccj.org/~smilczan/Two5/DR.html • http://www.science.uwaterloo.ca/~cchieh/cact/c120/reaction.html • http://www.citycollegiate.com/chapter2a.htm

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