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Powerpoint helps explain the Arrhenius equation.

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Multiple Choice Explanation Video

FRQ#1 Explanation Video

FRQ#2 Explanation Video

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just to make you laugh
https://www.youtube.com/watch?v=Veg63B8ofnQ
https://www.youtube.com/watch?v=Fc1P-AEaEp8
https://vine.co/v/eYz7hJhA9ij
https://www.youtube.com/watch?v=VVggXZPCuYw

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Multiple Choice Explanation Video
FRQ#1 Explanation Video
FRQ#2 Explanation Video

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- rare, simultaneous collisions of 3+ atoms
- 2A+B --> products, rate= k[A]^2[B]
- 3A --> products, rate = k[A]^3
- A+B+C --> products, rate = k[A][B][C]

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- 2 types
i. A+B --> products,  rate = k[A][B]
ii. 2A --> products, rate = k[A]^2
- can be the entire reaction or one step

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- A ---> products
- rate = k[A]
- may be one of elementary reactions or overall reaction
- reaction rate is directly proportional to concentration

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- reactions can only go as fast as the slowest step
- reaction mechanism must agree with experimentally determined rate law
- rate laws for elementary reactions can be written based on stoichiometry (only for elementary reaction)
-generally, if the rate-determining step is the first step in the mechanism, the rate law = the rate law for that step
- if the slow step does not equal the first step, and an equilibrium reaction is included in the mechanism:
~an equilibrium rxn is needed: A+B <---> C+D
~ K(subscript 1) -- forward reaction
~ K (subscript -1) -- reverse reaction
~K(subscript 1)[A][B] = K(subscript -1)[C][D]

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make sure you memorize this

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X+Y--->Z
Ea+ Δ G= activation energy of reverse reaction
- this reaction is exothermic

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The rate law is: rate = k
The integrated rate law is:
[A] = -kt + [A]o

k = rate constant that has units of 1/s

t = time

[A] = concentration of reaction or element at certain time

[A]o = initial concentration of reaction or element

The half life is:
t = [A]o/2k

t =half life

[A]o =initial concentration

k =rate constant

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The rate law is:
rate = k[A]^2
The integrated rate law is:
1/[A] = -kt + 1/[A]o

k = rate constant that has units of 1/s

t = time

1/[A] = inverse of concentration of reaction or element at certain time

1/[A]o =  inverse of initial concentration of reaction or element

The half life is:
t = 1/k[A]o

t =half life

[A]o =initial concentration

k =rate constant

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USING INITIAL RATES TO DETERMINE A RATE LAW (from chart):
1. determine m from data in which [A] varies but [B] remains the same
2. determine n from data where [B] varies but [A] stays the same
3. determine k using one set of concentrations and its corresponding rates

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Rate Law vs. Integrated Rate Law

Increasing Concentrations/Changing Exponents and how that impacts the rates

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** SUPER IMPORTANT
- 1st order: 1/s
- 2nd order:  1/ms
- 0 order: m/s

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The rate law is:
rate = k[X]
The integrated rate law is:

ln[X]= -kt + ln[X]o

k = rate constant that has units of 1/s

t = time

ln[X] = natural log of c oncentration of reaction or element at certain time

ln[X] = natural log of initial concentration of reaction or element

The half life is:
t = [A]o/2k

t = half life

[A]o = initial concentration

k = rate constant

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Click on the Image below to view the graphs.

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just a little teaser ;)

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Kinetics: Chemistry's Demolition Derby - Crash Course Chemistry #32

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- kinetics is all about the rate of reactions and the pathways the reactions take
- an increase in any of these will increase the rate of a reaction:
~concentration of reactions
~surface area of solid particles
~ temperature
~catalyst
- rates can be determined through the disappearance of reactants or the appearance of products
- doubling the exponent of a concentration increases the rate of a reaction four time
- Higher Ea means lower rate constant (slower rate), smaller e^(-Ea/RT) value (smaller fraction of molecules with enough energy to react), and vice versa
- turn arrhenius equation into linear equation form to calculate Ea
- a catalyst speeds up a reaction by lowering activation energy
~ homogeneous catalyst: present in same phase as reactants
~ heterogeneous catalyst: present in a different phase (usually solid) as the reactants
- if Ea is much greater than kinetic energy of the reactants, then the reaction will occur slowly, and vice versa

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https://quizlet.com/_2yb4wz