Practice HL: The Temperature Dependence of Rate: The Arrhenius Equation and Activation Energy - 5.6 | Module 5: Chemical Kinetics | IB Grade 12-Chemistry
K12 Students

Academics

AI-Powered learning for Grades 8–12, aligned with major Indian and international curricula.

Professionals

Professional Courses

Industry-relevant training in Business, Technology, and Design to help professionals and graduates upskill for real-world careers.

Games

Interactive Games

Fun, engaging games to boost memory, math fluency, typing speed, and English skills—perfect for learners of all ages.

Typing
Memory
Math
English Adventures
Knowledge

5.6 - HL: The Temperature Dependence of Rate: The Arrhenius Equation and Activation Energy

Enroll to start learning

You’ve not yet enrolled in this course. Please enroll for free to listen to audio lessons, classroom podcasts and take practice test.

Learning

Practice Questions

Test your understanding with targeted questions related to the topic.

Question 1

Easy

What is the Arrhenius equation used for?

💡 Hint: Think about reaction rates and temperature.

Question 2

Easy

What is the universal gas constant value in the Arrhenius equation?

💡 Hint: It’s a constant used for calculations in chemistry.

Practice 4 more questions and get performance evaluation

Interactive Quizzes

Engage in quick quizzes to reinforce what you've learned and check your comprehension.

Question 1

What does the Arrhenius equation model?

  • A relationship between pressure and volume
  • How temperature affects reaction rate
  • The solubility of gases

💡 Hint: Recall the topics we've covered on reaction kinetics.

Question 2

True or False: Higher activation energy means a faster reaction rate.

  • True
  • False

💡 Hint: Consider the meaning of activation energy.

Solve 1 more question and get performance evaluation

Challenge Problems

Push your limits with challenges.

Question 1

The rate constant for a chemical reaction is known to increase from 3.0 x 10^-5 to 1.2 x 10^-4 s^-1 as the temperature rises from 298 K to 308 K. Using the Arrhenius equation, calculate the activation energy (Ea).

💡 Hint: Find the natural log of the ratio of the rate constants and set up the equation to solve for Ea.

Question 2

A chemical reaction has an activation energy of 50 kJ/mol. How much faster will the reaction be at 350 K compared to 300 K based on the Arrhenius equation?

💡 Hint: Set up your calculations carefully, remembering to convert kilojoules to joules for R.

Challenge and get performance evaluation