Unit 5: Kinetics.
5.1 Reaction Rates.
Write the mathematical formula for the rate of appearance or
disappearance of a species in a chemical reaction as a change in
concentration over time, considering stoichiometric factors.
Justify how a chage in conditions (surface area, concentration/pressure,
temperature, presence of a catalyst) will affect the rate of the
reaction.
5.2 Introduction to Rate Law.
Know the meaning of zero, first, and second-order reactions.
-
What does it mean if a reaction is first-order with respect to [A]?
Write a rate law for a reaction using initial rate data from multiple
trials.
-
Determine the rate of the reaction: X + Y → XY
| Trial |
Initial [X] |
Initial [Y] |
Initial Rate of Appearance of XY Ms-1 |
| 1 |
0.01 |
0.01 |
0.005 |
| 2 |
0.01 |
0.02 |
0.010 |
| 3 |
0.02 |
0.01 |
0.025 |
Determine the overall order of the reaction by adding the powers of the
reactant concentrations in the rate law.
-
What is the overal order the reaction who's rate law is: rate =
k[A]2[B]?
Calculate the value of the rate constant (k) and express it with the
correct units.
Understand that the rate constant (k) is dependant on temperature and
therefore specific to a temperature.
-
If a reaction is increased from 300K to 400K would the rate constant
(k) increase, decrease, or remain constant?
5.3 Concentration Changes Over Time.
Determine the order of a reaction by examining graphs of [A] vs. t, ln
[A] vs. t, and 1/[A] vs. t.
Use the integrated rate law corresponding to the order of a reaction to
determine the value of k.
Recognize that the half-life of a first-order reaction is constant.
Apply the half-life equation for a first-order reaction to determine k
or the half-life of a reaction, including radioactive decay.
5.4 Elementary Reactions.
Use coefficients of elementary steps to determine the rate law.
5.5 Collision Model.
Use collision theory to justify whether a reaction will proceed under
given conditions.
Examine Maxwell-Boltzmann distributions to determine the likelihood of
successful collisions in a reaction.
5.6 Reaction Energy Profile.
Label the areas on a reaction energy profile: reactants, transition
state, products, activation energy.
Apply the Arrhenius equation qualitatively to discuss how temperature
affects the rate of an elementary reaction.
5.7 Introduction to Reaction Mechanisms.
Label the components of a reaction mechanism: reactants, products,
intermediates, catalysts.
Determine if a provided reaction mechanism is valid for a given
reaction.
5.8 Reaction Mechanism and Rate Law.
Use the slow step of a mechanism to write the rate law for the overall
reaction.
5.9 Pre-Equilibrium Approximation.
Use fast equilibrium expressions to substitute species in rate laws to
match an overall reaction description.
5.10 Multistep Reaction Energy Profile.
Draw a reaction energy profile with relative features that match given
conditions.
5.11 Catalysis.
Explain how a catalyst works.
Modify a reaction profile to show the effect of a catalyst.
Identify the presence of a covalent bond between a catalyst and a
reactant or intermediate.