91Ó°ÊÓ

How would you express the rate of the chemical reaction \(\mathrm{A} \rightarrow \mathrm{B}\) based on the concentration of Reactant \(\mathrm{A}\) ? How would that rate compare with the reaction rate based on the Product \(\mathrm{B}\) ?

What is the role of the activated complex in a chemical reaction?

Suppose two molecules that can react collide. Under what circumstances do the colliding molecules not react?

If \(\mathrm{A} \rightarrow \mathrm{B}\) is exothermic, how does the activation energy for the forward reaction compare with the activation energy for the reverse reaction \((\mathrm{A} \leftarrow \mathrm{B})\) ?

In the gas-phase reaction, \(\mathrm{I}_{2}+\mathrm{Cl}_{2} \rightarrow 2 \mathrm{ICl},\left[\mathrm{I}_{2}\right]\) changes from 0.400 \(\mathrm{M}\) at 0.00 \(\mathrm{min}\) to 0.300 \(\mathrm{M}\) at 4.00 \(\mathrm{min}\) . Calculate the average reaction rate in moles of I 2 consumed per liter per minute.

In a reaction \(\mathrm{Mg}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{H}_{2}(\mathrm{g})+\mathrm{MgCl}_{2}(\mathrm{aq})\) 6.00 \(\mathrm{g}\) of Mg was present at 0.00 \(\mathrm{min}\) . After 3.00 min, 4.50 \(\mathrm{g}\) of Mg remained. Express the average rate as mol Mg consumed/min.

If a chemical reaction occurs at the rate of \(2.25 \times 10^{-2}\) moles per liter per second at 322 \(\mathrm{K}\) , what is the rate expressed in moles per liter per minute?

What role does the reactivity of the reactants play in determining the rate of a chemical reaction?

In general, what is the relationship between reaction rate and reactant concentration?

Apply collision theory to explain why increasing the concentration of a reactant usually increases the reaction rate.