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Whatis ?
Effectivecollision?
Collisiontheory?
Factorsaffecting?
Activation
energy?
Energy level
diagram?
Rate of reaction
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What is the rate of a reaction
The rate of the reaction is howquickly the reaction happens.
Fast
reaction
Slowreaction
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Iron rusting - aCHEMICAL
REACTIONwith a slowreaction rate.
Wood burning -a chemical
reaction with afastreaction
rate.
http://en.wikipedia.org/wiki/Chemical_reactionhttp://en.wikipedia.org/wiki/Chemical_reactionhttp://en.wikipedia.org/wiki/Chemical_reactionhttp://en.wikipedia.org/wiki/Chemical_reactionhttp://en.wikipedia.org/wiki/Image:Large_bonfire.jpghttp://en.wikipedia.org/wiki/Image:Rust03102006.JPG -
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Whatis ?
Effectivecollision?
Collisiontheory?
Factorsaffecting?
Activation
energy?
Energy level
diagram?
Rate of reaction
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"You cant react if you dont collide."
collision theory
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1. the particles must collideto
react.
3 necessary requirements inorder for a reaction to take place:
2. Collision of particles mustproduceenough energy(to
overcome energy of activation)3. Collisions of particlesmust becorrectly oriented
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Whatis ?
Effectivecollision?
Collisiontheory?
Factorsaffecting?
Activation
energy?
Energy level
diagram?
Rate of reaction
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Prevent Effective collision
Camera to
detect fastmoving traffic
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Effective collision
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Whatis ?
Effectivecollision?
Collisiontheory?
Factorsaffecting?
Activation
energy?
Energy level
diagram?
Rate of reaction
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The energy that must beovercome in order for achemical reaction to occur
Activation energy is theminimum energy necessaryfor a specific chemicalreaction to occur
Activation energy
http://en.wikipedia.org/wiki/Chemical_reactionhttp://en.wikipedia.org/wiki/Chemical_reaction -
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The sparks generatedby striking steelagainst a flint provide
the activation energyto initiate combustionin this Bunsen
burner.
Activation energy
http://en.wikipedia.org/wiki/Ferroceriumhttp://en.wikipedia.org/wiki/Bunsen_burnerhttp://en.wikipedia.org/wiki/Bunsen_burnerhttp://en.wikipedia.org/wiki/Bunsen_burnerhttp://en.wikipedia.org/wiki/Bunsen_burnerhttp://en.wikipedia.org/wiki/Ferroceriumhttp://upload.wikimedia.org/wikipedia/commons/1/1b/Incandescence.jpg -
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A little
activationenergy is addedwith the aid of a
weed burner...
What is activation energy
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Not enoughkinetic energyfor reactants toleap over
reaction barrier.
A "hot" reaction inprogress showingreactants leapingover the activation
energy barrier
What is activation energy
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Activation energy
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Activation energy
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Only collisions with enough energy react to
form products.The critical amount of energy to make thereaction proceed
What is activation energy
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A + B C + D
reactants products
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What is activation energy
activation
energy
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Whatis ?
Effectivecollision?
Collisiontheory?
Factorsaffecting?
Activation
energy?
Energy level
diagram?
Rate of reaction
Wh t ff t th t f ti ?
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What affects the rate of a reaction?
Size ofreactant
Concentrationof reactants
/pressure
Temperatureof reactionmixture
catalyst
Wh ff h f i ?
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1. The effect of size of reactant
What affects the rate of a reaction?
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1. The effect of size of reactant
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THE EFFECT OF SIZE OF REACTANT
a reaction between magnesium metal and adilute acid like hydrochloric acid.
Increasing the number of collisions persecond increases the rate of reaction.
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Magnesium metal
THE EFFECT OF SIZE OF REACTANT
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Magnesium metal
THE EFFECT OF SIZE OF REACTANT
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1. The effect of size of reactant
Reducing the size of reactant
increases the Total Surface Area
increases the frequency of collisionsbetween particles
Increase the rate of reaction.
Increase the frequency effectivecollisions between particles
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2. Temperature
Increasing temperaturewill increase kinetic energy in the particles
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1. The effect of temperature
Increase the temperature of solution
increase the kinetic energy of particles
increase the frequency of collisionsbetween particles
Increase the rate of reaction.
Increase the frequency effectivecollisions between particles
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3. Concentration and Pressure
Increasing concentration or pressureincreases the number of particles per unit
volume
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1. The effect of concentration
Increase the concentration of solution
increase the number of particles perunit volume
increase the frequency of collisionsbetween particles
Increase the rate of reaction.
Increase the frequency effectivecollisions between particles
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- A catalyst will change the rate of areaction.- The catalyst itself does not take part
in the reaction - It is not changed bythe reaction- it is not used up during the reaction.
- A catalyst is usually a transitionmetal, a transition metal oxide
Properties of Catalysts
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4. Catalyst
How does a catalyst work?1) Provides a surface on which
the reaction can take place.2) This increases the number of
collisions between the
particles of the substancesthat are reacting.
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4. Catalyst
Often a catalyst is there to provide a
favourable surface for a reaction totake place
The blackobjectrepresents
thecatalyst
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Examples CATALYSTS
reaction catalyst
Decomposition of
hydrogen peroxide
manganese(IV)
oxide, MnO2Manufacture of ammonia
by the Haber Processiron
Contact Process to makesulphuric acid
vanadium(V)oxide, V2O5
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A catalyst provides an alternative routefor the reaction with a a lower activation
energy.
A ti ti ith t l t
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Activation energy with no catalyst
Activation energy with catalyst
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Activation energy with catalyst
4 The effect of catalyst
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4. The effect of catalyst
Catalyst provides alternative route
That has a lower activation energy
Increase the rate of reaction.
So more particles have energy equal orgreater than activation energy.
Number of effective collisions increase.
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Whatis ?
Effectivecollision?
Collisiontheory?
Factorsaffecting?
Activationenergy?
Energy level
diagram?
Rate of reaction
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End of
slides