IB Kinetics
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| Collision Theory | for a reaction to occur, two particles must collide with correct stereochemical orientation and sufficient energy (activation energy)
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| Increasing frequency of collisions | increases rate
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| rate determining step | slowest step
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| increase temperature | increase rate because particles move faster so there are more collisions per second and more particles will possess activation energy.
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| increase 10 degrees C | double rate of reaction
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| decrease temperature | decrease rate
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| increase surface area | rate increases because more particles can come in contact with reactant
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| decrease surface area | decrease rate
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| increase concentration | increase rate because there are more collisions per second
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| decrease concentration | decrease rate
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| catalyst | increases rate without being themselves chemically changed by providing an alternate pathway for reaction with a lower activation energy. More of the reactants possess this lower energy.
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| unimolecular process | single species breaking down into two or more products
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| biomolecular process | two species colliding and interacting
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| homogenous catalyst | same phase as reactants
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| hetergeneous catalyst | different phase as reactants
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