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Chemical Equations & Reactions Overview

Chapter 8 discusses chemical reactions, including identifying reactions, writing equations correctly, and balancing them. It covers reaction types like decomposition, combustion, single replacement, and double replacement. The chapter also explains reaction rates, factors affecting them, and the role of catalysts and inhibitors. Understanding these concepts is crucial in studying chemistry.

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Chemical Equations & Reactions Overview

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  1. Chapter 8: CHEMICAL EQUATIONS AND REACTIONS

  2. Indications of a Rxn • Heat or light given off • Bubbling/smoke, gas being released • Precipitate (solid) forms • Change in the odor/color • Chemical indicators turn color

  3. Eqn Writing Make sure you have the correct formula for each substance Diatomic elements – exist only in pairs, always written with a 2 subscript H2 O2 N2 Cl2 Br2 I2 F2

  4. Rxn/Eqn Parts H2 (g) + Cl2 (g)  2 HCl (g) Reactants Product (Reagents)

  5. Law of Conservation of Matter Atom values must match on both sides Balance an eqn with coefficient multipliers ___H2 + ___O2 ____ H2O 2 1 2

  6. ___Al2O3 ___ Al + __O2 2 4 3 1 3 3 1 __Fe(NO3)3 + __KSCN  __KNO3 + __Fe(SCN)3

  7. 5 Rxn Types

  8. Decomposition (analysis) One Reactantbreaking down into two or more products

  9. Combustion • One or more reactants combine with oxygen, O2 , must invole heat or light Usually takes place with carbon compounds and produces carbon dioxide and water CH4 + O2 CO2 + H2O

  10. Single Replacement (Displacement) • One element replaces a similar element in a compound

  11. Double Replacement • the interchanging of two ions from two different compounds. • Products usually have a precipitate

  12. Reaction rates The rate of disappearance of the reactants (concentration per second) Depends on activation energy and molecule collisions

  13. Factors affecting rate: • Type of reactants ion exchange happens quick covalent bond rearrangement is slow   2) Concentration and pressure higher amount increases the collision rate.

  14.  3) Temperature – increase it and collision rate increases 4) Catalysts – increases the rate by lowering activation energy 5) Inhibitors – used to slow rate, preservatives.

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