Practice Hl: Unveiling The Pathway: Reaction Mechanisms And The Rate Determining Step (5.5)

Practice: HL: Unveiling the Pathway: Reaction Mechanisms and the Rate Determining Step

Lesson 5.5Module 5: Chemical Kinetics

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8 questions

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6 sample questions

Question 1.
What is an elementary step?
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Think about the individual actions that contribute to the overall reaction.
Question 2.
Define intermediates.
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They are created and consumed during the reaction sequence.
3Question 3.
What is the rate-determining step?
- The fastest step in the mechanism
- The step that limits the overall reaction rate
- The first step of the reaction
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Consider which step controls the pace of the entire process.
4Question 4.
True or False: Intermediates appear in the overall balanced equation.
- True
- False
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Think about the lifecycle of intermediates in the reaction.
Question 5.
Consider a reaction where A + B → C occurs in two steps: Step 1 is A + B → D (slow) and Step 2 is D → C (fast). Write the rate expression and explain why the first step is rate-determining.
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Focus on the rate of the first step and how it influences the overall reaction.
Question 6.
A proposed mechanism for a reaction is: Step 1 (fast): A + B ↔ C (intermediate), Step 2 (slow): C + D → E. Derive the overall rate expression and give reasons for the steps identified.
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Remember that the RDS determines how we express the rate.

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