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Comments re Chapter 17 Problems:

17-1	Some T/F questions about rates and rate laws.
17-2	A question about the relationship between the form of the rate law and the units of the rate constant.
17-3	A short question about the relationship between rates for two reactants that have different stoichiometric coefficients.
17-9	A small thought problem that points out that rate constants are not rates.
17-25	A problem that is preparation for problems in which the rate law is determined from data about initial rates.
17-32 (not part c)	Determination of a rate law from information about initial rates. Calculate the rate constant for each set of concentrations and then average those rate constants for the best value. Note that rate constants are seldom known to much more than two digits.
17-44 (not part b)	Another problem in which a rate law is determined from information about initial rates. Very important.
17-10	An exercise in identifying the various components of a mechanism.
17-15	An exercise based on a first-order rate law. Applied calculus.
17-20	A small problem about an important distinction (same word used differently in two contexts)
17-22	How does the concentration of A change with time if the reaction is zero order?
17-40	Another short problem that emphasizes a very important distinction.
17-51	A small thought problem that emphasizes the low probability of three-body collisions.
17-59	Three T/F questions related to the Arrhenius equation.
17-62	Given the rate constant at two temperatures calculate Ea and then the pre-exponential factor A. Look at their values.
17-68	The relationship of Ea for the forward reaction, Ea for the reverse reaction, and DH^o (or DU^o, it doesn't really matter) for the overall reaction.
17-91	A T/F question about catalysts.
17-102	A problem concerning radioactive decay, which is always a first-order reaction. Note that the value for counts/s is the rate in atoms/s. The amount is given as mass rather than as a concentration because the substance is a solid so that the volume doesn't matter. It is necessary to change that mass to atoms of ^233U, which replaces the concentration (since the volume doesn't matter).
17-38	Problem based on the relationship Keq = kf/kr (microscopic reversibility). The problem is not as easy as it first looks because the stoichiometric coeffient is 1 for the reactant and 2 for the product. Note that the equilibrium constant must be calculated with molar concentrations rather than with pressures.
17-111	Yet another of Levine's excellent true-false problems.

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