unit 14 power point
TRANSCRIPT
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Activation Energy Activation Energy and Equilibriumand Equilibrium
Unit 14Unit 14
Insight Schools Insight Schools
Physical SciencePhysical Science
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Getting Chemical Reactions GoingGetting Chemical Reactions Going
EnergyEnergy is usually needed to break the bonds is usually needed to break the bonds and get the reaction going.and get the reaction going.
This can be a spark, This can be a spark,
flame, heat, or even a feather. flame, heat, or even a feather.
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Getting Chemical Reactions GoingGetting Chemical Reactions Going
Activation energy Activation energy is the term for the energy is the term for the energy needed to break the bonds so new bonds needed to break the bonds so new bonds can formcan form
Activation Energy
Energy Released Net
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Endothermic and Exothermic ReactionsEndothermic and Exothermic ReactionsExothermic Exothermic ReactionsReactions
Endothermic Endothermic ReactionsReactions
EnergyEnergy Energy is Released to Energy is Released to the surroundingsthe surroundings
Energy is Absorbed Energy is Absorbed from the surroundingsfrom the surroundings
SignsSigns Gets HotGets Hot
FlameFlame
LightLight
Gets ColdGets Cold
Dark colorDark color
ExamplesExamples Combustion of Combustion of MethaneMethane
Cold PackCold Pack
PhotosynthesisPhotosynthesis
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Factors That Influence Reaction RatesFactors That Influence Reaction RatesAffect on Reaction RateAffect on Reaction Rate
CatalystCatalyst Increases the Reaction Rate
Concentration of ReactantsConcentration of Reactants Increase in Concentration increases the reaction rate because of an increase in
particle collisions.
Surface AreaSurface Area More surface area increases the reaction rate. (Smaller particles give a greater
overall surface area when all the particles surfaces are added together.)
TemperatureTemperature Increase in Temperature increases the reaction rate because of an increase in
particle collisions.
StirringStirring Increases the Reaction Rate by increasing the number of collisions.
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Factors That Influence Reaction RatesFactors That Influence Reaction RatesAffect on Reaction RateAffect on Reaction Rate
CatalystCatalyst
Concentration of ReactantsConcentration of Reactants
Surface AreaSurface Area
TemperatureTemperature
StirringStirring
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The Affect of CatalystsThe Affect of Catalysts
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Exothermic vs EndothermicExothermic vs Endothermic
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EquilibriumEquilibriumThe point in a chemical reaction where the
rate at which reactants and products are being produced is equal.
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Equilibrium ConcentrationEquilibrium Concentration
Symbolized by [ ] around the compounds Symbolized by [ ] around the compounds or ionsor ions
[NaCl] [NaCl] [Na[Na++] and [Cl] and [Cl--]]H2O
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Changes in the Equilibrium Changes in the Equilibrium ConcentrationConcentration
Symbolized by [ ] around the compounds Symbolized by [ ] around the compounds or ionsor ions
[NaCl] [NaCl] [Na[Na++] and [Cl] and [Cl--]]
[NaCl] [NaCl] [Na[Na++] and [Cl] and [Cl--]]
[NaCl] [NaCl] [Na[Na++] and [Cl] and [Cl--]]
H2O
H2O evaporating
H2O added
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Changes in the Equilibrium ConcentrationChanges in the Equilibrium Concentration
[NaCl] [NaCl] [Na[Na++] and [Cl] and [Cl--]]
[NaCl] [NaCl] [Na[Na++] and [Cl] and [Cl--]]
H2O evaporating
H2O added
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Le Chatelier’s Le Chatelier’s PrinciplePrinciple
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Le Chatelier’s PrincipleLe Chatelier’s PrincipleIf something is done that disturbs a If something is done that disturbs a system at equilibrium, that system system at equilibrium, that system responds in a way to counteract what responds in a way to counteract what was done.was done.
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TemperatureTemperatureIncrease temperature:Increase temperature:
favors the endothermic reaction.favors the endothermic reaction.
Decrease temperature:Decrease temperature:
favors the exothermic reaction.favors the exothermic reaction.
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Pressure/Volume ChangesPressure/Volume ChangesIncrease pressure:Increase pressure: favors the reaction producing favors the reaction producing fewer moles of gas.fewer moles of gas.
Decrease pressure:Decrease pressure: favors the reaction producing favors the reaction producing more moles of gas.more moles of gas.
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Examples of Changes in EquilibriumExamples of Changes in Equilibrium
CO2
CO2
CO2
CO2
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Concentration ChangesConcentration Changes
Increase [reactant]:Increase [reactant]: favors favors the forward reactionthe forward reaction
Increase [product]:Increase [product]: favors favors the reverse reactionthe reverse reaction