Collision theory in chemical kinetics explains how the rate of chemical reactions is determined by the energy and orientation of colliding molecules. It highlights the importance of activation energy and molecular orientation for a successful reaction. Factors like temperature, concentration, and catalysts can influence reaction rates, with enzymes playing a crucial role in biological reactions.
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Collision theory explains the rate at which chemical reactions occur by positing that reactant molecules must collide with adequate energy and an appropriate orientation
Temperature and Concentration
Increasing temperature or reactant concentration can raise the frequency of collisions and accelerate reaction rates
Pressure and Surface Area
Increasing pressure or surface area can also increase the frequency of collisions and accelerate reaction rates
Catalysts
Catalysts lower the activation energy required for a reaction, allowing for a greater proportion of collisions to result in a reaction
Enthalpy diagrams illustrate the energy changes that occur during a chemical reaction, including the activation energy required for the reaction to proceed
The spatial arrangement of atoms during a molecular collision significantly influences the likelihood of a reaction
Activation energy is the minimum energy required for colliding molecules to result in a chemical reaction
Enzymes serve as natural catalysts in biological systems, reducing the activation energy required for biochemical reactions to occur
Exothermic reactions release energy, resulting in products with lower energy than the reactants
Endothermic reactions absorb energy, resulting in products with higher energy than the reactants
Enthalpy diagrams, also known as energy profiles, graphically depict the energy changes that occur during a chemical reaction
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In ______ theory, reactant molecules must collide with sufficient energy, called the ______ energy, and the right orientation to react.
Collision
activation
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Molecular collision and reaction likelihood
Proper alignment of atoms during collision increases reaction probability; incorrect alignment prevents reaction.
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Synthesis of bromoethane key interaction
Hydrogen from hydrogen bromide must approach ethene's double bond for successful bromoethane synthesis.
