Practice Integrated Rate Equations (4.6) - Chapter 4: Chemical Kinetics

Practice: Integrated Rate Equations

Lesson 4.6Chemical Kinetics

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9 questions

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6 sample questions

Question 1.
Define integrated rate equations and give an example of a zero-order reaction.
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Use the provided equation to set up your example.
Question 2.
What does it mean if a reaction is zero-order?
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Think about how concentration affects the reaction rate.
3Question 3.
What is the integrated rate equation for a zero-order reaction?
- [A] = [A]₀ - kt
- [A] = [A]₀e^(-kt)
- [A] = 1/[A]₀ + kt
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Remember that zero-order means the rate doesn't depend on concentration.
4Question 4.
True or False: The integrated rate equation for a first-order reaction can be expressed in logarithmic form.
- True
- False
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Consider how logarithms relate to exponential functions.
Question 5.
A first-order reaction has a half-life of 4 seconds. If the initial concentration was 2 M, what is the concentration after 12 seconds?
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Remember how to relate half-lives to concentration decreases.
Question 6.
In a zero-order reaction where the rate constant is 0.05 M/s, calculate the time required for the concentration to decrease from 1 M to 0.4 M.
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Carefully rearrange the equation to isolate t.

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