## Question

###### This reaction was monitored as a function of time: $$\mathrm{AB} \longrightarrow \mathrm{A}+\mathrm{B}$$ A plot of 1$/[\mathrm{AB}]$ versus time yields a straight line with slope $-0.055 / \mathrm{M} \cdot \mathrm{s} .$ \begin{equation} \begin{array}{l}{\text { a. What is the value of the rate constant }(k) \text { for this reaction at this }} \\ {\text { temperature? }}\\{\text { b. Write the rate law for the reaction. }} \\ {\text { c. What is the half-life when the initial concentration

This reaction was monitored as a function of time: $$\mathrm{AB} \longrightarrow \mathrm{A}+\mathrm{B}$$ A plot of 1$/[\mathrm{AB}]$ versus time yields a straight line with slope $-0.055 / \mathrm{M} \cdot \mathrm{s} .$ \begin{equation} \begin{array}{l}{\text { a. What is the value of the rate constant }(k) \text { for this reaction at this }} \\ {\text { temperature? }}\\{\text { b. Write the rate law for the reaction. }} \\ {\text { c. What is the half-life when the initial concentration is } 0.55 \mathrm{M} \text { ? }}\\{\text { d. If the initial concentration of } \mathrm{AB} \text { is } 0.250 \mathrm{M}, \text { and the reaction mixture }} \\ {\text { initially contains no products, what are the concentrations of } \mathrm{A} \text { and } \mathrm{B}} \\ {\text { after } 75 \mathrm{s} \text { ? }}\end{array} \end{equation}