Exam 2 Review
Chapter 14 (secs 14.5-14.6)
- What is the collision model of chemical reactions?
- What is the activation energy?
- What is an activated complex?
- Can you get a bottle of activated complex at the stockroom?
- Know how to draw and interpret energy profile diagrams
- What is meant by the mechanism of a reaction?
- What is an elementary step?
- What is meant by the molecularity of an elementary step?
- Be able to tell if an elementary step is unimolecular, bimolecular,
or termolecular
- What do the elementary steps in a multistep reaction mechanism have to add up to?
- How do we write rate laws for elementary processes?
- How do we determine rate laws for multistep mechanisms?
- Which step in a multistep mechanism is the rate-determining step?
- How do we deduce the rate law for a multistep mechanism for which the first
step is slow?
- When will intermediate appear in a rate law for an elementary step in a multistep mechanism?
- How and why do we assume equilibrium in a slow first step?
- How do we eliminate intermediates from rate laws using the assumption of equilibrium?
- Suggested problems: 43, 45,
53, 55, 57, 59, 87
Chapter 15
- When does chemical equilibrium occur?
- How are equilibrium constants related to kinetic rate constants for
elementary processes?
- How do we write equilibrium constant expressions for homogeneous reactions?
For heterogeneous reactions?
- To what side does the equilibrium position of a reaction lay if K >> 1? If
K << 1?
- Given the equilibrium constant for a reaction, be able to calculate the
equilibrium constant for the reverse reaction (or generally for a variation
of the reaction)
- Why don't pure solids and liquids appear in the equilibrium constant
expressions for heterogeneous reactions?
- How do we write equilibrium constant expressions for homogeneous reactions?
For heterogeneous reactions?
- To what side does the equilibrium position of a reaction lay if K >> 1? If
K << 1?
- Given the equilibrium constant for a reaction, be able to calculate the
equilibrium constant for the reverse reaction (or generally for a variation
of the reaction)
- Why don't pure solids and liquids appear in the equilibrium constant
expressions for heterogeneous reactions?
- How does one create an I-C-E table when working an equilibrium problem?
- Given a reaction, and the initial and equilibrium concentration of one species,
be able to calculate the value of K for the reaction.
- Given the value of K for a reaction, and the initial concentrations of one
or more species, be able to find the equilibrium concentrations of all species in
the reaction at equilibrium.
- What is meant by the reaction quotient, Q?
- How do we use Q to predict the direction a reaction will move to reach
equilibrium?
- Why does a reaction move to the left if Q > K? Why does a reaction move to
the right if K > Q?
- What is LeChatelier's principle?
- How does an equilibrium shift in response to added reactant? To added product?
- How does a heterogeneous equilibrium shift if some pure solid or pure liquid is added to or removed from
the equilibrium mixture?
- When does chaning total pressure on a gas-phase equilibrium cause the position of the equilibrium to shift?
- How does an equilibrium shift when heat is added to an endothermic reaction? An exothermic reaction?
- What is the effect of a catalyst on the position of chemical equilibrium?
Suggested problems: 15.8, 15.17, 21, 27, 29, 35, 43, 45, 47
Chapter 16 (16.1-16.6)
- What is an Arrhenius acid? An Arrhenius base?
- What is a Bronsted-Lowry acid/base?
- What is a conjugate acid/base pair?
- Given an acid, be able to deduce its conjugate base, and vice versa.
- How are the acid/base strengths of conjugate pairs related?
- What is meant by the autoionization of water?
- What is the equilibrium constant for the autoionization of water? What is
its value at 25oC?
- How is Kw used to calculate [H+] and [OH-] for a neutral solution?
- What is meant by an acidic solution? What is meant by a basic solution?
- Given [H+], how do we calculate [OH-] and vice versa?
- How is the pH scale defined?
- What are the strong acids?
- What are the strong bases?
- How does one calculate the pH of a strong acid?
- Given the pH of a strong acid, how does one calculate [H+]?
- How does one calculate the pH of a strong base?
- How are pH and pOH related?
- What is a weak acid?
- What is meant by the acid dissociation constant Ka?
- Be able to write the hydrolysis reaction for a weak acid in water.
- How do we use acid dissociation constants to gauge acid strength?
- How do we calculate the pH of weak acid solutions?
- What is meant by per cent ionization?
- When is it acceptable to 'neglect x'?
- What is a polyprotic acid?
- Which proton is generally more important in treating ionization of polyprotic
acids? Why?
Ch 16 suggested problems:
16.3, 16.5, 16.7, 16.9, 16.13, 16.19, 16.27, 31, 33, 41, 45, 49, 53,
55.
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