1. DE CHEMISTRY – King William High School

2.  1 mole = 6.02 x 10 23 particles  EX: How many molecules of CO 2 are in 1.75 moles?  EX: How many moles of carbon are in 1.50 moles of C 5 H 10 O 2 ?

3.  The amount of grams equal to one mole (decimal # from periodic table)  EX: What is the molar mass of aluminum oxide?  How many grams are in 0.500 moles of sodium chloride?

4.  Left of the arrow = reactants (what you start with)  Right of the arrow = products (what you end up with…what you make)  Must be balanced because of the Law of Conservation of Mass  EX: Fe 2 S 3 + HCL  FeCl 3 + H 2 S  EX: Na 3 PO 4 + MgCl 2  Mg 3 (PO 4 ) 2 + NaCl

5.  Synthesis (or combination)  one product  Decomposition  one reactant  Single replacement  one element + one compound on each side of the arrow  Double replacement  2 compounds on each side of the arrow  Combustion  oxygen is a reactant

6.  Electrons are transferred from one substance to another  OIL RIG  EX: Cu (s) + O 2 (g)  CuO (s)

7.  How many moles of sulfur are needed to react with 1.42 moles of iron? Fe (s) + S (s)  Fe 2 S 3 (s)

8.  How many grams of carbon dioxide are produced when 54.6 g of acetylene is burned? C 2 H 2 + O 2  CO 2 + H 2 O

9.  Exothermic – released of energy (energy is a product and  H is negative)  Endothermic – energy is absorbed (energy is a reactant and  H is positive)

10. How can you speed the rate of a reaction up???  Temperature (molecules move faster so there is a better chance that they collide and react)  Concentration (more collisions because more molecules in a given space)  Catalyst (lowers energy of activation)