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17 Cards in this Set

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example of fast reaction
explosion
example of slow reaction
decomposition of rust
rate
product/time
catalyst
lowers the energy of activiation-puts the particles together so you need less energy
endothermic reaction
A+energy-->CC
what does an endothermic reaction look like on the chart
lower at the beginning, higher at the end
exothermic reaction
A+B-->C + energy
what does an exothermic reaction look like on the chart
higher at the beginning, lower at the end
factors affecting rates of reaction
1. temperature-for every 10 degrees in temp, doubles the rate of reaction
2. concentration-adding particles will increase the rate
3. particle size-smaller particle size=larger surface area=faster reaction
4. catalyst-speeds up reaction-helps orient the molecules
5. inhibitor-slows down reaction
effective collisions
collisions must be effective in order for there to be a reaction
what two things are needed for the collision to be effective
1. colliding with adequate rate
2. correct angle
kinetics
the branch of chemistry considered with the rates and mechanics of reaction
princeton clock
clear--> yellow (intermediate)-->black
yellow shows intermediate product
rochelle salt and hydrogen peroxide- H2O2
-oxygen is reactive and kils germs when H2O2 breaks down
--kept in dark bottle because light causes it to break down
-colbalt chloride is a catalyst for the reaction-increases the rate of reaction but is not affected
-add peroxide to Rochelle salt-breaks down peroxide-
-end=water, colbalt chrloide
-shows how a catalyst works
rate determining step
the one that happens the slowest (only as fast as the slowest part)
what do rates measure
the speedof any change that occurs within an interval of time
collision theory
atoms, ions, and molecules can react to form products when they collide, provided that the particles have enough kinetic energy. particles lacking the necessary kinetic energy to react bouncees apart when they collide. collisions have to be effective