AP Chemistry
5.2 Introduction to Rate Law
The kinetics of the reaction between nitrogen monoxide gas and chlorine gas was investigated at \(300\text{ K}\):
\[ 2\text{NO}(g) + \text{Cl}_2(g) \rightarrow 2\text{NOCl}(g) \]
The reaction was determined to obey the rate law \(\text{rate} = k[\text{Cl}_2][\text{NO}]^2\), with a rate constant of \(k = 3.0 \times 10^2\text{ M}^{-2}\text{s}^{-1}\) at this temperature. If an experiment is initiated with \([\text{Cl}_2] = 0.050\text{ M}\) and \([\text{NO}] = 0.040\text{ M}\), what is the initial rate of the reaction?
\[ 2\text{NO}(g) + \text{Cl}_2(g) \rightarrow 2\text{NOCl}(g) \]
The reaction was determined to obey the rate law \(\text{rate} = k[\text{Cl}_2][\text{NO}]^2\), with a rate constant of \(k = 3.0 \times 10^2\text{ M}^{-2}\text{s}^{-1}\) at this temperature. If an experiment is initiated with \([\text{Cl}_2] = 0.050\text{ M}\) and \([\text{NO}] = 0.040\text{ M}\), what is the initial rate of the reaction?
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