Collision Theory Flashcards Preview

Chemistry 11.4 > Collision Theory > Flashcards

Flashcards in Collision Theory Deck (13)
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1
Q

what is the formula for reaction rate

A

amount of substance used or produced
—————————————-
Time Taken

2
Q

what happens as the gradient gets smaller

A

reaction slows down until it stops at 0

3
Q

what is the collision theory

A

describes chemical reaction in terms of collisions between individual reacting particles

4
Q

what are the 3 conditions that need to be met for a reaction to occur

A
  1. individual particles of reacting substance must collide
  2. collision energy but must greater than or equal to activation energy
  3. reacting particles must collide at suitable orientation
5
Q

what is the transition state

A

point at which original bonds are breaking while new bonds form - it is unstable and only exists for a short time until it decomposes and new products/original reactant form

6
Q

what does the potential energy profile show

A

the change in potential energy for reacting particles as the approach

7
Q

what is potential energy

A

the lost kinetic energy caused when the approaching particles repel (with enough KE, particles collide therefore have high potential enregy)

8
Q

what is the activation energy

A

minimum collision energy required to form transition state - higher when rectant bonds are strong because they need to break

9
Q

discuss hwo conentration affects reaction rate

A

increases amount of particles therefore increase change of possible collision

10
Q

discuss hwo gas pressure affects reaction rate

A

decreases volume of container, particles get closer therefore collision frequency increases

11
Q

discuss hwo temperature affects reaction rate

A

increased kinetic energy so more collsions have higher or equal activation energy therefore more collisions

12
Q

discuss hwo state of subdividsion affects reaction rate

A

particles only collide on surface so with higher surfae area reaction rate increases

13
Q

discuss hwo catalysts affects reaction rate

A

lowers actviation energy so more particles can achieve it