Reactant molecules MUST collide to produce a chemical reaction The concentrations of reactants...
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Transcript of Reactant molecules MUST collide to produce a chemical reaction The concentrations of reactants...
![Page 1: Reactant molecules MUST collide to produce a chemical reaction The concentrations of reactants affect the # of collisions among reactants For.](https://reader036.fdocuments.in/reader036/viewer/2022062321/56649e935503460f94b988b0/html5/thumbnails/1.jpg)
Collision Theory and Activation
Energy
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Reactant molecules MUST collide to produce a
chemical reaction The concentrations of reactants affect the # of
collisions among reactants For reactions occurring in one step—rate of
reaction is proportional to product of reactant concentrations Rate = k[A] [B]
Rate of any reaction step dependent on collision frequency
Collision Theory
![Page 3: Reactant molecules MUST collide to produce a chemical reaction The concentrations of reactants affect the # of collisions among reactants For.](https://reader036.fdocuments.in/reader036/viewer/2022062321/56649e935503460f94b988b0/html5/thumbnails/3.jpg)
1) Collision Rates between reactants
2) % of collisions with reactants arranged in proper orientation to produce reaction.
3) % of collisions with energy energy (activation energy) to produce reaction.
Variables Affecting Reaction Rate
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Increase in concentrations of reactants
Temperature increases
WHY?
When do collision rates increase?
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Small percentage of collisions actually convert
reactants to products. Why?
1) Molecular Orientation Random orientation Not all collisions have correct orientation
2) Molecular Energy at Collision Molecules have different kinetic energies Collision energy is energy source to get a reaction
started
Most collisions do NOT result in a chemical
reaction!
![Page 6: Reactant molecules MUST collide to produce a chemical reaction The concentrations of reactants affect the # of collisions among reactants For.](https://reader036.fdocuments.in/reader036/viewer/2022062321/56649e935503460f94b988b0/html5/thumbnails/6.jpg)
The amount of collision energy needed to
overcome Ea so the reaction can occur
Amount of energy needed for a chemical reaction to happen, energy needed to convert reactants to products.
Activation Energy (Ea)
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Activation Energy--Exothermic
![Page 8: Reactant molecules MUST collide to produce a chemical reaction The concentrations of reactants affect the # of collisions among reactants For.](https://reader036.fdocuments.in/reader036/viewer/2022062321/56649e935503460f94b988b0/html5/thumbnails/8.jpg)
Activation Energy--Endothermic
![Page 9: Reactant molecules MUST collide to produce a chemical reaction The concentrations of reactants affect the # of collisions among reactants For.](https://reader036.fdocuments.in/reader036/viewer/2022062321/56649e935503460f94b988b0/html5/thumbnails/9.jpg)
1) MUST have a collision
2) Collision must happen with the correct molecular orientation to generate a reaction
3) Collision energy ≥ Ea
When will reactions occur?
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HOW?
Temperature increases reaction
rate.
![Page 11: Reactant molecules MUST collide to produce a chemical reaction The concentrations of reactants affect the # of collisions among reactants For.](https://reader036.fdocuments.in/reader036/viewer/2022062321/56649e935503460f94b988b0/html5/thumbnails/11.jpg)
Rate constant and reaction rate are
temperature dependent.
Enables the activation energy for a reaction to be determined based on the relationship between reaction rate and temperature.
Arrhenius Equation
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lnk = -Ea ( 1/T ) + lnA
R k = rate constant Ea = activation energy (J) R = 8.314 J/molK T = Kelvin Z = proportionality constant, changes based on reaction
Arrhenius Equation
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Different form of equation can be used to
observe how temperature changes affect the rate constant (k)
ln (k1/k2) = Ea (1/T2 – 1/T1)
R
Arrhenius Equation
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Calculate activation energy (Ea) for HI
decomposition with the following data.
Example 1
Temperature (K) Rate Constant (M/s)
573 2.91 x 10-6
673 8.38 x 10-4
773 7.65 x 10-2