Chemical Kinetics

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Brief summary of things to know about Chemical Kinetics for the MCAT

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Chemical Kinetics
  1. Gibb's Free Energy
    1. spontaneity of reaction: Positive=not spontaneous Negative=spotaneous
      1. + DG => endergonic- consumes energy -DG=> exergonic- gives off energy
    2. Collision Theory:
      1. rate of reaction is proportional to the number of collisions per second btw the reacting molecules. They must be in the correct orientation and energy.
      2. Transition State Theory:
        1. when molecules collide with energy higher than the activation energy, they form a transition state in which old bonds are weakened by new bonds forming.
        2. Factors affecting reaction rate:
          1. *reaction concentrations *Temperature *medium (polar solvents etc.) *catalysts
          2. Reaction Orders
            1. Zero Order:
              1. rate=k[A]^0 [B]^0=k
              2. First Order:
                1. rate=k[A]^1
                2. Second Order:
                  1. rate=k[A]^1[B]^1 or rate=k[A]^2
                  2. Mixed Order: reactions that change order over time
                    1. rate=k1[C][A]^2/k2=k3[A]
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