ch 9 and 10 rates of reaction and extent of reaction Flashcards
whatre the 2 ways you can work out the rate of a chemical reaction
reactants used up/time
amount of products formed/time
steeper slope =
faster reaction
what is collision theory
particles must collide with a certain amount of energy before they can react
what is activation energy
the minimum amount of energy that particles must have in order to react
how does having a larger surface affect reaction rate
it increases it because more particles from the product are exposed to reactants so the frequency of collisions increases
what are the 4 factors that affect rate of reaction
-temperature
-surface area
-concentration or pressure
-catalyst
what happens to particles when temperature decreases
-particles colide more slowly with less energy so rate of reaction decreases
what happens to particles when temperature inceceases
paticles colide more frequently with more energy so theres a greater chance of successful collisions
what affect does increasing concentration or pressure have on a reaction
it increases the frequency of collisions because there are more reactant particles moving in the same volume which increases the chance of a successful collision
what is a catalyst
a substance that increases the rate of reaction without being used up
how do catalyst speed up rate of reaction
they create an alternate pathway which is shorter than activation energy
whats a reversable reaction
a reaction that can go in both ways so the products can react again to remake the reactants
what is chemical equilibrium,
when the rate of forward and backward reaction are equal in a closed system
suggest why some solids form closer to one end than other (3)
diffusion happens faster because the substance diffuses towards another faster since it has a smaller mr
explain why a reaction is endothermid in terms of bond breaking and making (3)
energy taken in is larger than energy taken out so more energy is taken in that given out so more energy is takken in by the surroudings
