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Stephanie Yeung Per. 3 (Kinetics (factors affecting rate (surface area,…

- - - - rate = M/s
      - k = rate constant (M/s)
      - n = reactant order
      - [] = reactant concentration (M)
    - - k = rate/[A]n[B]n
  - - - Δ[A] = concentration 2 - concentration 1
      - Δt = t2 - t1
      - reactant is negative (used up)
      - coefficient of reactant multiplies to Δt
      - product is positive (being made)
- - - - x = coefficents in balanced equation
      - [] = concentration (M)
      - K = equilibrium constant
    - - if Q = K, system is at equilibrium
      - if Q < K, system shifts right until equilibrium
      - if Q > K, system shifts left until equilibrium
  - - - I: initial concentrations
      - C: change, - for reactants, + for product, multiplied by coefficient in balanced equation, symbol is x
        
        solve for x - plug in values in the law of mass action -move terms to one side ordered by ax2 +bx + c, plug in quadratic formula
      - E: equilibrium concentrations, add to change
  - - - pressure
        
        pressure increase - system shifts to the side with fewer moles in the balanced equation
        
        pressure decrease - system shifts to the side with more moles in the balanced equation
      - concentration of the reactants or products
        
        adding reactant - more products are produced to offset the gain of reactant; system shifts left
        
        removing reactant - more reactants are produced to offset the loss of reactant; system shifts right
      - temperature
        
        temperature increase - endothermic reaction: heat on reactant side moves to product side to remove some of added energy; system shifts right
        
        temperature increase - exothermic reaction: heat on product side moves to reactant side to remove some of added energy; system shifts left