Kinetics
A lower activation energy can help increase the number of effective collisions. Which of the following contributes to that?
What sets an ineffective collision apart from an effective collision? (A) there isn't enough force, (B), molecules move too slowly, (C), molecules aren't aligned right.
What factor does NOT affect the rate of reaction as predicted by the collision model?
How does adding a catalyst affect the rate of chemical reactions according to the collision model?
How does the activation energy (Ea) of a reaction influence the reaction rate according to the collision model?
What is the effect on activation energy when a catalyst provides an alternative pathway for a chemical reaction according to collision theory?
What would happen to the rate of reaction if the particles were at a higher temperature according to the collision model?
How are we doing?
Give us your feedback and let us know how we can improve
When more particles have a greater energy than it's activation energy, what happens to the reaction rate?
How does increasing the temperature affect the rate of a chemical reaction according to the collision model?
Why might increasing surface area lead to an increased reaction rate based on collision theory?