AP Chemistry
5.6 Reaction Energy Profile
5.5 Collision Model
A student investigates the rate of the gas-phase decomposition of nitrogen dioxide represented by the equation below:
\[ 2\text{NO}_2\text{(g)} \rightarrow 2\text{NO(g)} + \text{O}_2\text{(g)} \]
When the temperature of the reaction vessel is increased from \(300\text{ K}\) to \(320\text{ K}\) at constant volume, the measured initial reaction rate increases by a factor of approximately \(4\), whereas the calculated total frequency of molecular collisions increases by only about \(3\%\). Which of the following best explains why the reaction rate increases so significantly compared to the collision frequency?
\[ 2\text{NO}_2\text{(g)} \rightarrow 2\text{NO(g)} + \text{O}_2\text{(g)} \]
When the temperature of the reaction vessel is increased from \(300\text{ K}\) to \(320\text{ K}\) at constant volume, the measured initial reaction rate increases by a factor of approximately \(4\), whereas the calculated total frequency of molecular collisions increases by only about \(3\%\). Which of the following best explains why the reaction rate increases so significantly compared to the collision frequency?
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