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IB Kinetics

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Question
Answer
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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