CHEM 162 Exam 3 Review
page 1 of 4
CHEM 162: Exam 3 Study Guide
CHAPTER 15: Chemical Kinetics
chemical kinetics:
study of the factors that
influence reaction rates
reaction rate:
a
positive
quantity expressing the
concentration change with time
Use experimental data given to
–
determine a general reaction rate given
concentrations of reactants/products over time
–
determine the rate of disappearance/
consumption of a reactant or rate of
appearance/production of a product given the
rate of disappearance/appearance of another
reactant/product in the reaction
Determine reaction rate
–
Given experimental data of concentrations and
time.
Know the terms:
rate law, rate constant (k)
Reaction Order
:
–
zero
‐
order, first
‐
order, second
‐
order
–
Determine overall order for a reaction given rate
law.
Distinguish between the
instantaneous reaction
rate
and the
average reaction rate
.
Determine rate law
using
initial rates method
–
Given data of concentrations and rates.
–
Cannot be determined given only the balanced
chemical equation.
half
‐
life (t
1/2
):
the time required for the
concentration of a reactant to decrease by half
Determine the reaction order
given
experimental
data
of
reactant concentration over time
.
–
Recognize the
plots
giving a straight line for
zero
‐
order, first
‐
order,
and
second
‐
order
reactions.
Determine the reaction order
given
experimental
data
of
reactant concentration over time
(Continued)
–
Recognize that the
half
‐
life is only constant
for
first
‐
order reactions
.
–
Compare slopes for the first and last sets of data
to see if slope changes for each reaction order.
Do calculations
given
integrated rate laws
for
zero
‐
order, first
‐
order,
and
second
‐
order
reactions.
–
Solve for concentration at a given time given
initial concentration and rate constant.
–
Carry out natural log (ln) calculations for 1
st
‐
order reactions—review your algebra!
–
Solve for the time required for the
concentration to decrease to a given amount.
–
Solve for half
‐
life given rate constant, k, or vice
versa.
COLLISION MODEL/THEORY:
reactant molecules
must collide to react
Activation Energy (E
a
):
minimum energy needed
for chemical reaction
Reaction Rate and Temperature
–
As T
, reaction rate
since molecules move
faster and more molecules have activation
energy.
This preview has intentionally blurred sections. Sign up to view the full version.
View Full Document
This is the end of the preview.
Sign up
to
access the rest of the document.
 Fall '11
 Jake
 Chemistry, Periodic Table, Reaction, Christopher Nolan, Nuclear magnetic resonance, Kelvins

Click to edit the document details