Chapter 16: Kinetics: Rates and Mechanism of Chemical Reactions

(a) What is the difference between an average rate and an instantaneous rate? (b) What is the difference between an initial rate and an instantaneous rate?

Give two reasons to measure initialrates in a kinetic study.

Express the rate of reaction in terms of the change in concentration of each of the reactants and products:

$\mathbf{2}\mathbf{D}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{3}\mathbf{E}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{F}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{\to }\mathbf{2}\mathbf{G}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{H}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

When [D] is decreasing at 0.1 mol/L.s, how fast is [H] increasing?

The rate constant of a reaction is $\mathbf{4}\mathbf{.}\mathbf{7}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{3}}\mathbf{}{\mathbf{s}}^{\mathbf{-}\mathbf{1}}$at $\mathbf{25}{\mathbf{}}^{\mathbf{0}}\mathbf{C}$, and the activation energy is 33.6 kJ/mol. What is k at $\mathbf{75}{\mathbf{}}^{\mathbf{0}}\mathbf{C}$?

The rate constant of a reaction is $\mathbf{4}\mathbf{.}\mathbf{50}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{5}}\mathbf{}\mathbf{L}\mathbf{/}\mathbf{mol}\mathbf{.}\mathbf{s}$at $\mathbf{195}{\mathbf{}}^{\mathbf{0}}\mathbf{c}$and $\mathbf{3}\mathbf{.}\mathbf{20}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{3}}\mathbf{}\mathbf{L}\mathbf{/}\mathbf{mol}\mathbf{.}\mathbf{s}$ at $\mathbf{258}{\mathbf{}}^{\mathbf{0}}\mathbf{C}$ . What is the activation energy of the reaction?

What is the central idea of collision theory? How does this idea explain the effect of concentration on reaction rate?