AP Chemistry
5.8 Reaction Mechanism and Rate Law
5.7 Introduction to Reaction Mechanisms
A proposed mechanism for the gas-phase reaction \(2\,\text{NO}_2\text{(g)} + \text{F}_2\text{(g)} \rightarrow 2\,\text{NO}_2\text{F(g)}\) consists of the following two elementary steps:
Step 1: \(\text{NO}_2\text{(g)} + \text{F}_2\text{(g)} \rightarrow \text{NO}_2\text{F(g)} + \text{F(g)}\) (slow)
Step 2: \(\text{NO}_2\text{(g)} + \text{F(g)} \rightarrow \text{NO}_2\text{F(g)}\) (fast)
Which of the following claims and justifications best explains why the experimentally observed rate law is \(\text{Rate} = k[\text{NO}_2][\text{F}_2]\)?
Step 1: \(\text{NO}_2\text{(g)} + \text{F}_2\text{(g)} \rightarrow \text{NO}_2\text{F(g)} + \text{F(g)}\) (slow)
Step 2: \(\text{NO}_2\text{(g)} + \text{F(g)} \rightarrow \text{NO}_2\text{F(g)}\) (fast)
Which of the following claims and justifications best explains why the experimentally observed rate law is \(\text{Rate} = k[\text{NO}_2][\text{F}_2]\)?
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