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Rates and Equilibrium (Chemical rates (Calculate reaction rates/ Rate Law:…

- - - - Temperature: Increases kinetic energy in molecules = more effective collision chances from faster moving particles
      - Concentration: more molecules = higher chance of effective collisions
      - Surface area: A higher SA = more particles colliding in a given time ---> speeds up reactions
  - - - Example:
        
        2x= 2
        
        x = 1
        
        2x =4
        
        x = 2
        
        [A]
        
        [B]
        
        Not very clear description
- - - - When the reactants (N2 and 3H2) synthesize, ammonia is produced. This is the forward reaction since the reactants synthesize to form a product.
    - - When the product (2NH3) breaks down or is combined, the reactants (N2 and 3H2) will be produced.
  - - - Equilibrium Constant: "K" what is solved for using the equilibrium constant expression
        
        This value is only constant at a specified temperature :star:
        
        K < 1: Reactants are favored at equilibrium (More reactants are yielded)
        
        K > 1: Products are favored at equilibrium (More products are yielded)
        
        how do you solve equilibrium problems?
        
        you were asked to provide source for all images
  - - - Step 1.) Assume reaction goes 100% to products or reactants
      - Step 2.) Make an ICE table (Initial concentration, change in concentration, equilibrium concentration)
      - Step 3.) Solve for x and assume it is very small
      - Step 4.) Check work by plugging the equilibrium concentrations back into the K/Equilibrium constant expression
  - - - Stress: Any kind of change in a system that upsets equilibrium.
      - Increase Concentration of a Substance = Shift away from the substance
      - Decrease in concentration = towards the substance
      - Increase in pressure of a system = towards fewer moles of gas
      - Decrease pressure of a system = towards more moles of gas
      - Increase temperature of system = Away from heat/energy (endothermic reaction is favored)
      - Decrease temperature of system = towards heat/energy (exothermic reaction favored)