AP Chemistry
5.8 Reaction Mechanism and Rate Law
5.7 Introduction to Reaction Mechanisms
A student investigates the kinetics of the gas-phase reaction represented by the balanced equation below:
\[2\text{NO}_2\text{(g)} + \text{F}_2\text{(g)} \rightarrow 2\text{NO}_2\text{F(g)}\]
A proposed mechanism for the reaction consists of two elementary steps:
\[\text{Step 1: } \text{NO}_2\text{(g)} + \text{F}_2\text{(g)} \rightarrow \text{NO}_2\text{F(g)} + \text{F(g)} \quad (\text{slow})\]
\[\text{Step 2: } \text{NO}_2\text{(g)} + \text{F(g)} \rightarrow \text{NO}_2\text{F(g)} \quad (\text{fast})\]
If the initial concentration of \(\text{NO}_2\text{(g)}\) is doubled while the initial concentration of \(\text{F}_2\text{(g)}\) and the temperature remain constant, which of the following correctly predicts the effect on the initial rate of the reaction?
\[2\text{NO}_2\text{(g)} + \text{F}_2\text{(g)} \rightarrow 2\text{NO}_2\text{F(g)}\]
A proposed mechanism for the reaction consists of two elementary steps:
\[\text{Step 1: } \text{NO}_2\text{(g)} + \text{F}_2\text{(g)} \rightarrow \text{NO}_2\text{F(g)} + \text{F(g)} \quad (\text{slow})\]
\[\text{Step 2: } \text{NO}_2\text{(g)} + \text{F(g)} \rightarrow \text{NO}_2\text{F(g)} \quad (\text{fast})\]
If the initial concentration of \(\text{NO}_2\text{(g)}\) is doubled while the initial concentration of \(\text{F}_2\text{(g)}\) and the temperature remain constant, which of the following correctly predicts the effect on the initial rate of the reaction?
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