Practice Second-order Reactions (4.3.3) - Unit 6: Chemical Kinetics - IB 11 Chemistry

Practice: Second-Order Reactions

Lesson 4.3.3Unit 6: Chemical Kinetics

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8 questions

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Exercise
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6 sample questions

Question 1.
What is the rate equation for a second-order reaction involving two molecules of A?
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Use the definition of second-order reactions.
Question 2.
How does the half-life of a second-order reaction depend on the initial concentration?
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Think about how the formula for half-life is constructed.
3Question 3.
What is the rate law for a second-order reaction involving two different reactants?
- Rate = k[A]²
- Rate = k[A][B]
- Rate = k[A]³
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Remember how different reactants interact in second-order kinetics.
4Question 4.
True or False: The half-life for second-order reactions decreases as the initial concentration increases.
- True
- False
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Consider how the rate of reaction changes with different initial concentrations.
Question 5.
A sample of a second-order reaction at time zero contains A at 0.6 M. If after 4 seconds the concentration drops to 0.3 M, find the rate constant k.
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Use the integrated rate law to set up the calculation.
Question 6.
In a second-order reaction involving A + B → products, the system starts with [A]_0 = [B]_0 = 0.1 M. Calculate how long it would take for [A] to drop to 0.05 M if k = 3 M^-1 s^-1.
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Apply the correct values to the integrated rate law.

4 more questions in this section. Enroll free to practise them all.