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Questions and Answers
What must happen for a chemical reaction to occur, according to collision theory?
What must happen for a chemical reaction to occur, according to collision theory?
The particles involved must collide with each other.
What is the minimum amount of energy that particles need to react called?
What is the minimum amount of energy that particles need to react called?
Activation energy
What are the four main ways to increase reaction rates?
What are the four main ways to increase reaction rates?
- Decrease the volume of the reactants
- Increase the surface area of solid reactants (correct)
- Increase the temperature of the reactants (correct)
- Increase the concentration of reactants (correct)
- Add a catalyst (correct)
A dilute solution has a large amount of solute in a small amount of solvent.
A dilute solution has a large amount of solute in a small amount of solvent.
Increasing the temperature of reactants decreases the rate of reaction.
Increasing the temperature of reactants decreases the rate of reaction.
What is the function of a catalyst in a chemical reaction?
What is the function of a catalyst in a chemical reaction?
What is an example of a biological catalyst?
What is an example of a biological catalyst?
What is an inhibitor in a chemical reaction?
What is an inhibitor in a chemical reaction?
What is an example of an inhibitor?
What is an example of an inhibitor?
Flashcards
Activation Energy
Activation Energy
The minimum amount of energy needed for particles to react and form products.
Collision Theory
Collision Theory
A theory explaining chemical reactions, stating particles need to collide with sufficient energy to overcome the activation energy.
Rate of Reaction
Rate of Reaction
The speed at which a chemical reaction takes place.
Energy Changes in Reactions
Energy Changes in Reactions
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Catalyst
Catalyst
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Enzyme
Enzyme
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Surface Area
Surface Area
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Concentration
Concentration
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Temperature
Temperature
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Concentration
Concentration
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Inhibitor
Inhibitor
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Study Notes
Reaction Energy
- Bonds between atoms in reactants must be broken, requiring energy absorption.
- New bonds forming in products release energy.
Collision Theory
- Chemical reactions require particle collisions.
- Collisions must possess sufficient energy (activation energy) to overcome a barrier.
- Reaction rate depends on the frequency of energy-sufficient collisions.
- Activation energy is the minimum energy particles need to react.
Collision Model
- Molecules must collide to react.
- Collisions must have enough energy to break existing bonds and form new ones.
- Successful collisions form products.
Factors Affecting Reaction Rates
- Surface Area: Increased surface area of solid reactants leads to faster reactions.
- Concentration: Higher concentration of reactants increases the number of collisions and thus reaction rate.
- Temperature: Higher temperatures increase particle movement, increasing collision frequency and energy, accelerating reaction rate.
- Catalysts: Catalysts speed up reactions by lowering the activation energy needed for particles to react. Catalysts aren't consumed in the process. Enzymes are biological catalysts.
Dilute vs. Concentrated Solutions
- Dilute solutions have a small amount of solute in a large amount of solvent.
- Concentrated solutions have a large amount of solute in a small amount of solvent.
Inhibitors
- Inhibitors decrease the rate of a chemical reaction.
- Antioxidants are an example.
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