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U10 PT - Cam (Chemical Rates (Reaction Rates (The change in concentration…

- - - - More particles to collide, frequency of successful collisions increase, reaction rates increase
    - - Increase the kinetic energy of the particles, making them collide more frequently, more successful collisions, so reaction rates increase
    - - Increase the S.A will allow particles collide with more particles over a unit of time, increasing the reaction rates
  - - - rate = k [A][B]
        
        A and B are reactants
  - - - The sum of the exponent values in the rate law equation
    - - Can be determined using the Initial Rates Method
        
        Shows how the rate of a reaction is affect by the concentration of a reactant
- - - - Keq = [A]^a [B]^b / [C] ^ c
        
        a, b, c are the coefficients of a balanced equation
        
        Equilibrium of synthesis of ammonia: [NH3]^2 / [N2] [H2]^3
  - - - x is very small that it could be assumed to be zero
        
        it could be ignore, not assumed to be equal toz ero
      - I (Initial): reactants is a positive value, products are 0
      - C (Change): change by the factor (x), reactants have negative value, products have positive values
      - E (Equilibrium): The sum of the Initial and the Change
      - Plug the values of Equilibrium back to the Equilibrium Expression, find the missing data
  - - - Increase Temperature
        
        Shifts away from the heat
        
        Exothermic reaction
        
        reactants favored since heat is the product side
        
        Example: N2 + 3H2 <=> 2NH3 + heat
        
        Endothermic reaction
        
        products favored since heat is the reactant
        
        Example: N2O4 + heat <=> 2 NO2
      - Increase Pressure
        
        Shift to the side with less gas molecules
      - Increase Concentration
        
        Shift away from the species was added
      - Adding a catalyst
        
        No shifts at all