AP Chemistry
5.6 Reaction Energy Profile
5.5 Collision Model
A student investigates the gas-phase reaction represented by the equation below in a rigid container.
\[ 2\text{ NOCl(g)} \rightarrow 2\text{ NO(g)} + \text{Cl}_2\text{(g)} \]
When the temperature of the system is increased from \(300\text{ K}\) to \(310\text{ K}\), the initial rate of the reaction approximately doubles, while the total number of molecular collisions per second increases by only about \(1.7\%\). Which of the following best explains why the reaction rate increases so substantially despite the minor increase in total collision frequency?
\[ 2\text{ NOCl(g)} \rightarrow 2\text{ NO(g)} + \text{Cl}_2\text{(g)} \]
When the temperature of the system is increased from \(300\text{ K}\) to \(310\text{ K}\), the initial rate of the reaction approximately doubles, while the total number of molecular collisions per second increases by only about \(1.7\%\). Which of the following best explains why the reaction rate increases so substantially despite the minor increase in total collision frequency?
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