- The reactant concentration in a zero-order reaction was $7.00×10^{−2}~\mathrm{M}$ after $160~\mathrm{s}$ and $2.50×10^{−2}~\mathrm{M}$ after $345~\mathrm{s}$. What is the rate constant for this reaction?
- What was the initial reactant concentration for the reaction described in part one?
- The reactant concentration in a first-order reaction was $7.70×10^{−2}~\mathrm{M}$ after $50.0~\mathrm{s}$ and $1.60×10^{−3}~\mathrm{M}$ after $85.0~\mathrm{s}$. What is the rate constant for this reaction?
Background info: The integrated rate laws for zero and first order reactions may be arranged such that they resemble the equation for a straight line, $y=mx+b$.
\begin{array}{lccc} \text{Order}& \text{Integrated Rate Law}& \text{Graph}& \text{Slope} \\\hline 0 & [A]=−kt+[A]_0 & [A]\text{ vs. }t & −k\\ 1 & \ln[A]=−kt+\ln[A]_0 & \ln[A]\text{ vs. }t & −k\\\hline \end{array}