AP Chemistry
5.2 Introduction to Rate Law
The reaction between \(\text{NO(g)}\) and \(\text{Cl}_2\text{(g)}\) proceeds according to the equation below.
\[ 2\text{NO(g)} + \text{Cl}_2\text{(g)} \rightarrow 2\text{NOCl(g)} \]
Based on experimental data, the reaction is first order with respect to \(\text{Cl}_2\text{(g)}\) and second order with respect to \(\text{NO(g)}\). In a second trial conducted at the same temperature, the initial concentration of \(\text{Cl}_2\text{(g)}\) is doubled and the initial concentration of \(\text{NO(g)}\) is tripled. By what factor does the initial rate of the reaction increase?
\[ 2\text{NO(g)} + \text{Cl}_2\text{(g)} \rightarrow 2\text{NOCl(g)} \]
Based on experimental data, the reaction is first order with respect to \(\text{Cl}_2\text{(g)}\) and second order with respect to \(\text{NO(g)}\). In a second trial conducted at the same temperature, the initial concentration of \(\text{Cl}_2\text{(g)}\) is doubled and the initial concentration of \(\text{NO(g)}\) is tripled. By what factor does the initial rate of the reaction increase?
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