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- https://chem.libretexts.org/Courses/University_of_Arkansas_Little_Rock/Chem_3572%3A_Physical_Chemistry_for_Life_Sciences_(Siraj)/Text/09%3A_Chemical_Kinetics/9.07%3A_Theories_of_Reaction_RatesThe macroscopic discussion of kinetics discussed in previous sections can be now expanded into a more microscopic picture in terms of molecular level properties (e..g, mass and velocities) involving t...The macroscopic discussion of kinetics discussed in previous sections can be now expanded into a more microscopic picture in terms of molecular level properties (e..g, mass and velocities) involving two important theories: (1) collision theory and (2) transition-state theory.
- https://chem.libretexts.org/Courses/Indiana_Tech/EWC%3A_CHEM_1000_-_Introductory_Chemistry_(Budhi)/15%3A_Chemical_Equilibrium/15.02%3A_The_Rate_of_a_Chemical_ReactionThe rate, or speed, at which a reaction occurs depends on the frequency of successful collisions. Remember, a successful collision occurs when two reactants collide with enough energy and with the rig...The rate, or speed, at which a reaction occurs depends on the frequency of successful collisions. Remember, a successful collision occurs when two reactants collide with enough energy and with the right orientation. That means if we can do things that will increase the number of collisions, increase the number of particles that have enough energy to react and/or increase the number of particles with the correct orientation we will increase the rate of a reaction.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/Book%3A_Structure_and_Reactivity_in_Organic_Biological_and_Inorganic_Chemistry_(Schaller)/IV%3A__Reactivity_in_Organic_Biological_and_Inorganic_Chemistry_2/01%3A_Reaction_Kinetics/1.04%3A_Collisions_and_PhaseIn the drawing below, the cold, sluggish molecules on the left don't appear to be in danger of colliding with anything, but the hot, zippy molecules on the right look like they are due for a crash at ...In the drawing below, the cold, sluggish molecules on the left don't appear to be in danger of colliding with anything, but the hot, zippy molecules on the right look like they are due for a crash at any time. The disadvantage of using a solvent is that the solvent must be removed at the end of the reaction, so that the desired product can be isolated and used.
- https://chem.libretexts.org/Courses/Thompson_Rivers_University/TRU%3A_Fundamentals_and_Principles_of_Chemistry_(CHEM_1510_and_CHEM_1520)/04%3A_Kinetics/4.06%3A_Collision_TheoryChemical reactions require collisions between reactant species. These reactant collisions must be of proper orientation and sufficient energy in order to result in product formation. Collision theory ...Chemical reactions require collisions between reactant species. These reactant collisions must be of proper orientation and sufficient energy in order to result in product formation. Collision theory provides a simple but effective explanation for the effect of many experimental parameters on reaction rates. The Arrhenius equation describes the relation between a reaction’s rate constant and its activation energy, temperature, and dependence on collision orientation.
- https://chem.libretexts.org/Courses/University_of_British_Columbia/CHEM_100%3A_Foundations_of_Chemistry/15%3A_Chemical_Equilibrium/15.02%3A_The_Rate_of_a_Chemical_ReactionThe rate, or speed, at which a reaction occurs depends on the frequency of successful collisions. Remember, a successful collision occurs when two reactants collide with enough energy and with the rig...The rate, or speed, at which a reaction occurs depends on the frequency of successful collisions. Remember, a successful collision occurs when two reactants collide with enough energy and with the right orientation. That means if we can do things that will increase the number of collisions, increase the number of particles that have enough energy to react and/or increase the number of particles with the correct orientation we will increase the rate of a reaction.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Kinetics/06%3A_Modeling_Reaction_Kinetics/6.01%3A_Collision_Theory/6.1.06%3A_The_Collision_TheoryCollision theory explains why different reactions occur at different rates, and suggests ways to change the rate of a reaction. Collision theory states that for a chemical reaction to occur, the react...Collision theory explains why different reactions occur at different rates, and suggests ways to change the rate of a reaction. Collision theory states that for a chemical reaction to occur, the reacting particles must collide with one another. The rate of the reaction depends on the frequency of collisions. The theory also tells us that reacting particles often collide without reacting.
- https://chem.libretexts.org/Courses/Pacific_Union_College/Kinetics/08%3A_Chemical_Kinetics/8.07%3A_Theories_of_Reaction_RatesThe macroscopic discussion of kinetics discussed in previous sections can be now expanded into a more microscopic picture in terms of molecular level properties (e..g, mass and velocities) involving t...The macroscopic discussion of kinetics discussed in previous sections can be now expanded into a more microscopic picture in terms of molecular level properties (e..g, mass and velocities) involving two important theories: (1) collision theory and (2) transition-state theory.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/18%3A_Kinetics/18.06%3A_Factors_Affecting_Reaction_RateThis page discusses the stress of driving on crowded freeways and the factors affecting chemical reaction rates. High traffic contributes to driving stress, while in chemistry, factors like concentrat...This page discusses the stress of driving on crowded freeways and the factors affecting chemical reaction rates. High traffic contributes to driving stress, while in chemistry, factors like concentration, pressure, surface area, and temperature are crucial for reaction speeds. Increased concentration and pressure enhance collision frequency, smaller particles improve surface area, and higher temperatures accelerate particle movement, all contributing to faster reactions.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(LibreTexts)/15%3A_Chemical_Equilibrium/15.02%3A_The_Rate_of_a_Chemical_ReactionThe rate, or speed, at which a reaction occurs depends on the frequency of successful collisions. Remember, a successful collision occurs when two reactants collide with enough energy and with the rig...The rate, or speed, at which a reaction occurs depends on the frequency of successful collisions. Remember, a successful collision occurs when two reactants collide with enough energy and with the right orientation. That means if there is an increase in the number of collisions, an increase in the number of particles that have enough energy to react, and/or an increase in the number of particles with the correct orientation, the rate of reaction will increase.
- https://chem.libretexts.org/Courses/Knox_College/Chem_322%3A_Physical_Chemisty_II/01%3A_Chemical_Kinetics/1.07%3A_Theories_of_Reaction_RatesThe macroscopic discussion of kinetics discussed in previous sections can be now expanded into a more microscopic picture in terms of molecular level properties (e..g, mass and velocities) involving t...The macroscopic discussion of kinetics discussed in previous sections can be now expanded into a more microscopic picture in terms of molecular level properties (e..g, mass and velocities) involving two important theories: (1) collision theory and (2) transition-state theory.
- https://chem.libretexts.org/Ancillary_Materials/Worksheets/Worksheets%3A_Inorganic_Chemistry/Worksheets%3A_Structure_and_Reactivity_in_Organic_Biological_and_Inorganic_Chemistry/1%3A_Reaction_Kinetics/1.4%3A_Collisions_and_PhaseIn the drawing below, the cold, sluggish molecules on the left don't appear to be in danger of colliding with anything, but the hot, zippy molecules on the right look like they are due for a crash at ...In the drawing below, the cold, sluggish molecules on the left don't appear to be in danger of colliding with anything, but the hot, zippy molecules on the right look like they are due for a crash at any time. The higher the temperature, the more mobile the molecules will be, and the more likely they are to collide and react. The disadvantage of using a solvent is that the solvent must be removed at the end of the reaction, so that the desired product can be isolated and used.
