Practice Understanding The Relationship Within The Arrhenius Equation (5.6.1) - Module 5: Chemical Kinetics

Practice: Understanding the Relationship within the Arrhenius Equation

Lesson 5.6.1Module 5: Chemical Kinetics

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8 questions

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3 cards from this section. Quick, good the night before a test.
Exercise
6 questions · about 4 min · pass mark 70%. Hints available.
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Quiz
2 questions · about 1 min · pass mark 70%. Hints available.
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6 sample questions

Question 1.
What does the Arrhenius equation relate to in chemical reactions?
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Think about the factors affecting how fast reactions occur.
Question 2.
What happens to reaction rates when temperature increases?
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Consider the molecular motion and energy distribution.
3Question 3.
What effect does increasing temperature have on the rate constant (k)?
- Decreases k
- Increases k
- Has no effect on k
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Think about the energy distribution of molecules.
4Question 4.
True or False: Higher activation energy always leads to faster reaction rates.
- True
- False
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Consider the concept of energy barriers.
Question 5.
Given that the rate constant for a particular reaction is measured at 400 K and found to be 0.0025 s^-1, while at 500 K it is 0.067 s^-1, calculate the activation energy.
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Break the problem into smaller parts and ensure units are consistent.
Question 6.
Explain how using a catalyst in a reaction alters the Arrhenius parameters described in the equation.
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Focus on how energy barriers change with and without catalysis.

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