PRELIMINARY COURSE ASSESSMENT

CHEMISTRY:

REACTION RATES

 

HOMEPAGE

PART A

PART B

PART C

BIBLIOGRAPHY

TEAM MEMBERS

GUEST BOOK

ABOUT

 

 

Q.

a) The importance of collisions between reacting particles, and *

b) the need for safety in work environments where fine particles mix with air. 

 

Page: 3 of 10 (* currently answering part (a) )

 

Example 2

 

NO + O3 ® NO2 + O2

This reaction is a forward reaction and only occurs in one step. Its rate of reaction depends on the frequency collisions between NO and O3 and is therefore proportional to the concentration of No and O3.

 In order for collisions to be effective, there must be considerable force in the collisions.  The slower moving molecules do not have enough kinetic energy to react when they collide and instead they bounce off one another and retain their identity.

Only those molecules moving at high speed have enough energy for collisions to result in a reaction.

Example 3

 

H2 + I2 ® 2HI

   

Doubling the concentration of H2 will double the amount of product. Similarly, doubling the concentration of I2 will also double the amount of the product HI.

Doubling both the amounts of H2 and I2 will quadruple the amount of product formed.

 

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