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Reaction Rates

cava chem 303 s2d48 5.01 Reaction Rates

QuestionAnswer
Reactants [...] together in reactions. Reactants collide together in reactions.
When the reactants collide with sufficient speed and the proper orientation, they don't immediately form the [...]. When the reactants collide with sufficient speed and the proper orientation, they don't immediately form the products.
When the reactants collide with sufficient speed and the proper orientation, they form an [...] complex. When the reactants collide with sufficient speed and the proper orientation, they form an activated complex.
After forming, the activated complex then breaks apart to form the [...]. After forming, the activated complex then breaks apart to form the products.
The energy difference between the activated complex and the reactants is called the [...] energy. he energy difference between the activated complex and the reactants is called the activation energy.
Reactant molecules must have [...] energy to form products. Reactant molecules must have activation energy to form products.
According to collision theory, any factor that can cause more [...] of reactant molecules or cause more molecules to have energies greater than the activation energy will increase the rate of reaction. According to collision theory, any factor that can cause more collisions of reactant molecules or cause more molecules to have energies greater than the activation energy will increase the rate of reaction.
If more reactant molecules are crowded together in the same volume, the frequency of [...] will increase. If more reactant molecules are crowded together in the same volume, the frequency of collision will increase.
Increasing [...] increases the average kinetic energy of the reactant molecules and the reaction rate. Increasing temperature increases the average kinetic energy of the reactant molecules and the reaction rate.
[-er] particles have greater surface areas for more collisions (and higher reaction rates). Smaller particles have greater surface areas for more collisions (and higher reaction rates).
Higher [...] forces reactant molecules closer together and increases the frequency of collisions (and therefore, the reaction rate). Higher pressure forces reactant molecules closer together and increases the frequency of collisions (and therefore, the reaction rate).
A [...] increases the rate of a system's reactions without being used up itself. A catalyst increases the rate of a system's reactions without being used up itself.
A catalyst increases the reaction rate by lowering the [...] of a chemical reaction. A catalyst increases the reaction rate by lowering the activation energy of a chemical reaction.
Created by: mr.shapard