Collision Theory Of Chemical Reactions
Chapter Name : Chemical Kinetics |
Sub Topic Code : 102_12_04_07_01 |
Topic Name : Collision Theory Of Chemical Reactions |
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Sub Topic Name : Collision Theory Of Chemical Reactions |
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Introduction
The collisions in which molecules collide with sufficient kinetic energy and proper orientation, so as to facilitate breaking of bonds between reacting species and formation of new bonds to form products are called as effective collisions.
Pre-Requisites:
Effective collision, factors affecting rate of chemical reaction
Activity:
Powdered zinc reacts to form hydrogen gas faster than large pieces of zinc when both are placed in hydrochloric acid.
Real Life Question:
How would the collision theory apply to the rugby?
Key Words / FlashCards
| Key Words | Definitions (pref. in our own words) |
|---|---|
| Effective collision | Collision between the reactant molecules resulting in the formation of products. |
| Collision frequency | The number of collisions per second per unit volume of the reaction mixture is known as collision frequency. |
Learning aids / Gadgets
| Gadgets | How it can be used |
|---|
Real life uses :
Powdered zinc reacts to form hydrogen gas faster than large pieces of zinc when both are placed in hydrochloric acid.
Places to visit :
Labs
Practical examples around us
| Examples | Explainations |
|---|---|
| Addition of vinegar to baking soda | When vinegar is added to the baking soda the fizzing and bubbling of the reaction requires the collision theory. |
What you learn in Theory:
When reactant molecules collide they may react together or they may not, depending on two factors : 1. Proper Orientation 2. Threshold Energy
What you learn in Practice:
In collision theory activation energy and proper orientation of the molecules together determine the criteria for an effective collision and hence the rate of a chemical reaction.