AP Chemistry
5.8 Reaction Mechanism and Rate Law
5.7 Introduction to Reaction Mechanisms
5.2 Introduction to Rate Law
A chemist investigates the reaction between nitrogen dioxide and carbon monoxide represented by the following balanced equation:
\[ \text{NO}_2(g) + \text{CO}(g) \rightarrow \text{NO}(g) + \text{CO}_2(g) \]
Two different mechanisms are proposed for the reaction:
Mechanism 1 (single elementary step):
\[ \text{NO}_2(g) + \text{CO}(g) \rightarrow \text{NO}(g) + \text{CO}_2(g) \]
Mechanism 2 (two-step mechanism):
\[ \text{Step 1 (slow): } 2\,\text{NO}_2(g) \rightarrow \text{NO}_3(g) + \text{NO}(g) \]
\[ \text{Step 2 (fast): } \text{NO}_3(g) + \text{CO}(g) \rightarrow \text{NO}_2(g) + \text{CO}_2(g) \]
Which of the following experimental results would provide the most decisive evidence to support Mechanism 2 over Mechanism 1?
\[ \text{NO}_2(g) + \text{CO}(g) \rightarrow \text{NO}(g) + \text{CO}_2(g) \]
Two different mechanisms are proposed for the reaction:
Mechanism 1 (single elementary step):
\[ \text{NO}_2(g) + \text{CO}(g) \rightarrow \text{NO}(g) + \text{CO}_2(g) \]
Mechanism 2 (two-step mechanism):
\[ \text{Step 1 (slow): } 2\,\text{NO}_2(g) \rightarrow \text{NO}_3(g) + \text{NO}(g) \]
\[ \text{Step 2 (fast): } \text{NO}_3(g) + \text{CO}(g) \rightarrow \text{NO}_2(g) + \text{CO}_2(g) \]
Which of the following experimental results would provide the most decisive evidence to support Mechanism 2 over Mechanism 1?
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