Stoichiometry

            Avogadro’s number = 6.022 X 10²³

Gases

            for all the equations:

            n = no. of moles                         T = absolute temperature

            P = pressure                             R = ideal gas constant = 0.082 L.atm/K.mol

Ideal Gas Equation:  PV = nRT

General Gas Law

       P_1­V_{1     =}          P₂V₂
           T₁                         T₂

            at constant temperature  P_1­V₁ = P_2­V₂        Boyle’s Law

            at constant pressure   V_{1  =}  V₂                Charles’ Law
                                              T₁    T₂

            at constant temperature  P_{1  =}  P₂            Gay-Lussac’s Law
                                                  T₁      T₂

STP₂  Standard Temperature & Pressure, 0⁰C and 1 atm

-          at STP 1 mole of any gas has a volume of 22.4L

Gas Diffusion

            - lighter gases diffuse faster than heavier gases

Palton’s Law of Partial Pressure

-          the sum of the partial pressure of all the components in a gas mixture is equal to the total pressure 

P_T   =  P_a  +  P_b  +  P_c  + …

Concentration of Solutions

molarity, M           M = moles  of  solute
                                  Liters of solution

molality, M           M = moles  of  solute
                                  kilograms of solvent

mole fraction, x    x =    moles   of component
                                      total mole of solution

Periodic table trends

Increasing ionization potential, electron affinity, electronegativity, and non-metallic character

                        A + B   ---------      AB

2. Decomposition

AB       ---------      A + B

3. Single Replacement

                        A + BX    ---------    AX + B

4. Double Replacement/ Double Decomposition

                        AX + BY   ---------    AY + BX

Factors affecting the rate of a chemical reaction

1. nature of the reactants

2. temperature – the higher the temperature, the faster the reaction

3. concentration – the higher the concentration of the reactants, the faster the reaction

4. surface area – the greater the exposed surface area, the faster the reaction

5. presence of a catalyst

Redox Reactions

Ways to identify Oxidation & Reduction

electrochemical cell – uses redox reactions to produce or use electricity

Types of electrochemical cells:

1. electrolytic cell – uses electricity to start a non-spontaneous redox reaction

2. voltaic or galvanic cell – uses a spontaneous redox reaction to produce electricity