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Questions and Answers
A chemist observes that increasing the temperature of a reaction increases the rate of the reaction. According to collision theory, which statement BEST explains this observation?
A chemist observes that increasing the temperature of a reaction increases the rate of the reaction. According to collision theory, which statement BEST explains this observation?
- At higher temperatures, reactant particles are more likely to collide with sufficient energy to overcome the activation energy barrier. (correct)
- Increasing the temperature introduces a catalyst, which lowers the activation energy.
- At higher temperatures, reactant particles are more likely to collide with the correct orientation.
- At higher temperatures, the concentration of reactants increases, leading to more frequent collisions.
A student conducts an experiment where they react marble chips (calcium carbonate) with hydrochloric acid. Which of the following changes would NOT increase the rate of reaction?
A student conducts an experiment where they react marble chips (calcium carbonate) with hydrochloric acid. Which of the following changes would NOT increase the rate of reaction?
- Increasing the concentration of the hydrochloric acid.
- Adding a catalyst to the reaction mixture.
- Lowering the temperature of the reaction. (correct)
- Decreasing the size of the marble chips.
Consider a reaction in which two molecules must collide with a specific orientation to react. Which of the following would MOST effectively increase the rate of this reaction?
Consider a reaction in which two molecules must collide with a specific orientation to react. Which of the following would MOST effectively increase the rate of this reaction?
- Increasing the concentration of the reactants while decreasing the temperature.
- Decreasing the concentration of the reactants while increasing the temperature.
- Decreasing the surface area of the reactants.
- Introducing a catalyst that aligns the molecules in the correct orientation. (correct)
In a chemical reaction, only a small fraction of collisions leads to product formation. What is the primary reason for this?
In a chemical reaction, only a small fraction of collisions leads to product formation. What is the primary reason for this?
A reaction is carried out in two trials. In the first trial, the reaction is complete in 60 seconds. In the second trial, with a change to the reaction conditions, it is complete in 30 seconds. What can be concluded about the rate of reaction in the second trial, compared to the first?
A reaction is carried out in two trials. In the first trial, the reaction is complete in 60 seconds. In the second trial, with a change to the reaction conditions, it is complete in 30 seconds. What can be concluded about the rate of reaction in the second trial, compared to the first?
Which of the following scenarios would MOST likely lead to an increase in the number of successful collisions in a chemical reaction?
Which of the following scenarios would MOST likely lead to an increase in the number of successful collisions in a chemical reaction?
A student is investigating the rate of reaction between zinc granules and sulfuric acid. They conduct several experiments, changing one variable at a time. Which change would NOT increase the rate of hydrogen gas production?
A student is investigating the rate of reaction between zinc granules and sulfuric acid. They conduct several experiments, changing one variable at a time. Which change would NOT increase the rate of hydrogen gas production?
A chemical company wants to optimize a reaction in a large industrial reactor. According to collision theory, which combination of factors would BEST achieve this?
A chemical company wants to optimize a reaction in a large industrial reactor. According to collision theory, which combination of factors would BEST achieve this?
Why does increasing the surface area of a solid reactant typically increase the rate of a chemical reaction?
Why does increasing the surface area of a solid reactant typically increase the rate of a chemical reaction?
Two reactions are performed: Reaction A has a high activation energy, and Reaction B has a low activation energy. Assuming all other factors are equal, which of the following statements is most likely true?
Two reactions are performed: Reaction A has a high activation energy, and Reaction B has a low activation energy. Assuming all other factors are equal, which of the following statements is most likely true?
Flashcards
Rate of Reaction
Rate of Reaction
Measures how fast reactants become products.
Collision Requirement
Collision Requirement
Particles must come into contact for reaction.
Energy Requirement
Energy Requirement
Particles need enough energy to break bonds.
Orientation Requirement
Orientation Requirement
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Successful Collision
Successful Collision
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Increased Reaction Rate
Increased Reaction Rate
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Factors Affecting Reaction Rate
Factors Affecting Reaction Rate
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Time vs Rate
Time vs Rate
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Study Notes
- Rate of reaction refers to how quickly reactants turn into products.
- A chemical reaction needs colliding particles.
- For a chemical reaction to occur these steps must be met.
- Particles must collide with each other.
- Particles must collide with sufficient energy to break bonds between reactants.
- Particles must collide with the correct orientation, enabling reactant bonds to break and new bonds to form.
- Meeting the above steps leads to a successful collision.
- Most collisions do not end in a chemical reaction.
- Reactions need successful collisions to occur.
- Increasing the number of successful collisions per second increases the rate of reaction.
- Factors that affect the reaction rate: temperature, surface area, concentration, and catalysts.
- As reaction time decreases, the reaction rate increases.
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