AP Chemistry
5.5 Collision Model
A student investigates the gas-phase reaction between nitrogen monoxide and ozone:
\[ \text{NO(g)} + \text{O}_3\text{(g)} \rightarrow \text{NO}_2\text{(g)} + \text{O}_2\text{(g)} \]
When the temperature of the reaction mixture is increased from \(298\text{ K}\) to \(310\text{ K}\) at constant volume, the rate of the reaction increases by more than a factor of \(2\), even though the total collision frequency between reactant molecules increases by only about \(2\%\). Which of the following best explains why the reaction rate increases so substantially?
\[ \text{NO(g)} + \text{O}_3\text{(g)} \rightarrow \text{NO}_2\text{(g)} + \text{O}_2\text{(g)} \]
When the temperature of the reaction mixture is increased from \(298\text{ K}\) to \(310\text{ K}\) at constant volume, the rate of the reaction increases by more than a factor of \(2\), even though the total collision frequency between reactant molecules increases by only about \(2\%\). Which of the following best explains why the reaction rate increases so substantially?
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