The document discusses the collision theory of reaction rates. It explains that for a reaction to occur, reactant particles must collide with enough kinetic energy to overcome the activation energy barrier. Factors that increase collisions such as higher concentrations, temperatures, and surface areas can increase the reaction rate by providing more opportunities for effective collisions that yield products. Catalysts also increase the reaction rate by lowering the activation energy required for collisions to be effective.
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The Roman Empire, a vast and enduring power, stands as one of history's most remarkable civilizations, leaving an indelible imprint on the world. It emerged from the Roman Republic, transitioning into an imperial powerhouse under the leadership of Augustus Caesar in 27 BCE. This transformation marked the beginning of an era defined by unprecedented territorial expansion, architectural marvels, and profound cultural influence.
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The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
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1. Effective from September 2015 | Plus term chemistry Wk6 – session 1
Joanne Lumley
Week 6 – session 1
Rates of Reactions
2. Effective from September 2015 | Plus term chemistry Wk6 – session 1
In Contact
• Reactions
don’t happen
unless the
substances
are in contact.
3. Effective from September 2015 | Plus term chemistry Wk6 – session 1
Why?
• The particles of
the reactants
need to get
together so
that they can
react.
4. Effective from September 2015 | Plus term chemistry Wk6 – session 1
How?
Reactant particles
collide
Product particles
formed
REACTION
5. Effective from September 2015 | Plus term chemistry Wk6 – session 1
Not all collisions are effective
• Paper burns
• Paper + oxygen carbon dioxide + water + nitrogen
• The paper in this room isn’t burning.
• It doesn’t have enough energy to burn.
• If we make it hotter it will catch fire.
• Paper burns on its own at 250 ºC
6. Effective from September 2015 | Plus term chemistry Wk6 – session 1
A collision but with no effect
Reactant particles
collide
Product particles
not formed as there is not
enough energy
7. Effective from September 2015 | Plus term chemistry Wk6 – session 1
Activation Energy
• Reactions only
happen if the
particles have
enough energy.
• The minimum amount
of energy needed to
start a reaction is called
the Activation Energy
• The amount of
activation energy
needed is different for
each reaction.
• But
• Every reaction has
activation energy,
they all need a little
push to get started.
8. Effective from September 2015 | Plus term chemistry Wk6 – session 1
More than the activation energy.
Reactant particles
collide
Product particles
formed
REACTION
9. Effective from September 2015 | Plus term chemistry Wk6 – session 1
More than the activation energy.
C
O O
CO O
Effective collisions, a reaction.
10. Effective from September 2015 | Plus term chemistry Wk6 – session 1
The Collision Theory
• Particles are constantly moving
• For a chemical reaction to take place the reactant
particles must collide first
• For the collision to be effective the particles must have
the right amount of energy
• The minimum amount of energy required for an
effective collision is called the activation energy
11. Effective from September 2015 | Plus term chemistry Wk6 – session 1
Factors affecting rate
• Concentration
• Temperature
• Catalysts
• Surface Area
12. Effective from September 2015 | Plus term chemistry Wk6 – session 1
Concentration
• More particles in the same space means more collisions.
• More collisions means more effective collisions
• If we double the concentration we double the number of
collisions
13. Effective from September 2015 | Plus term chemistry Wk6 – session 1
Temperature
• Particles turn heat energy into kinetic energy
• When they get hotter they move faster
• When they move faster they collide more often
• More collisions means more effective collisions
14. Effective from September 2015 | Plus term chemistry Wk6 – session 1
Catalysts
• Catalysts reduce the activation energy needed for a reaction
• They do this by offering an alternate route for the reaction to
take
• Less activation energy means more effective collisions
• More effective collisions means faster rate
Activation energy
with a catalyst
15. Effective from September 2015 | Plus term chemistry Wk6 – session 1
Surface Area/Particle Size
• Using smaller particles increases rate
• Increase in surface area allows more collisions at surface
• More collisions means more effective collisions means faster
rate.
