Unit 4.1 kinetics Flashcards
inert gas
gas that does not react with other substances bc it is stable so no chemical reactions
ex- helium, argon
what happens if an inert gas is added to a reaction?
nothing lol
adding an inert gas does not affect the rate or equilibrium yes or no
ya adding an inert gas does not affect the rate or equilibrium bc it doesn’t participate in reaction stuff
catalysts
increases the rate of a chemical reaction without being consumed.
also lowers activation energy obviously
and allows for more successful collisions
what are the 3 types of catalysts
biological catalysts, homogeneous catalysts, heterogeneous catalysts
biological catalysts
enzymes are special proteins that are specific to substrates like they do this in humans and plants
homogeneous catalysts
-they stay in the same phase (state) as the reactants
-they work bc theyre in the same phase and can mix easily with reactants which make the reactions happen faster
like putting more water in batter to make it more flowy and easier to stir
heterogeneous catalysts
-catalysts in a different phase form the reactants.
-catalysts and solid, reactants are liquid or gas
-they work by the reactants coming in contact with the catalyst and speeds it up but they never mix together
like how rocks help a river flow faster
temp and reaction rate rule of thumb
10 degrees celcius increase will double the reaction rate
collision theory
-a reaction happens when particles collide with enough energy (activation energy) and the correct orientation
-increasing the concentration of reactants or raising the temperature increases collision rates, this increasing the reaction rate
-more frequent or energetic collisions lead to faster reactions
how does a catalyst affect the rate of a chemical reaction?
it lowers the activation energy, leading to a more successful collisions and faster reaction rate
what energy do particles need to collide
transitional energy (their movement) to convert vibrational energy to bond together so they hit hard enough they stick together
when collisions meet all their criteria to bond thats called
effective collisions
criteria for effective collisions
-enough energy
-correct orientation
activation complex
after particles collide with enough energy, they form activated complex which is like the highest energy point (peak of the curve)
at this state they can continue and form products or fall back to original reactants
reaction rate formula
rate= change in concentration / time interval
rate=M/sec
is the rate constant
no
instantaneous reaction rate
finding the rate at a specific time
how to find instantaneous reaction rate
1) draw a tangent line at the point on the graph youre interested in
2) find the y-int and thats the M
3) find the x int where the line ends and thats sec
4) then do M/sec
5)units are Ms^-1
what is relative reaction rate
the rate at which reactants disappear or products appear in a reaction
relative reaction rate for a reactant
rate is always negative since its disappearing
relative reaction rate for a product
rate is always positive since its forming
relative reaction rate formulas
ex- 2NO2–> O2 + 2NO
divide each coefficient into a fraction and make reactants neg and products pos
and put each one equal to each other and divided by triangle t
-1/2 ▲[NO2] / ▲ t = ▲[O2]/▲t =
1/2 ▲[NO] /▲t
what is the rate constant
K, it tells us how fast the reaction goes
