3.5 - Collision Theory of Chemical Reactions
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.
Practice Questions
Test your understanding with targeted questions
What is activation energy?
💡 Hint: Think about the energy barrier needed for a reaction to happen.
Define collision frequency.
💡 Hint: Consider how often reactant molecules meet each other.
4 more questions available
Interactive Quizzes
Quick quizzes to reinforce your learning
What does the Collision Theory state about reactions?
💡 Hint: Think about what makes a collision 'effective'.
True or False: Higher temperature decreases the reaction rate.
💡 Hint: Recall how temperature affects molecular motion.
1 more question available
Challenge Problems
Push your limits with advanced challenges
Given that the collision frequency for a reaction is 3.5 x 10^9 collisions per liter per second, and the activation energy is 50 kJ/mol at a certain temperature, calculate the rate of the reaction if the temperature is raised by 10 K.
💡 Hint: Don't forget to convert the activation energy into J/mol and use the appropriate values for R.
Discuss how increasing pressure in a gaseous reaction influences collision frequency and the rate of reaction.
💡 Hint: Think about how the volume change relates to pressure and how this impacts molecular interactions.
Get performance evaluation
Reference links
Supplementary resources to enhance your learning experience.