AP Chemistry
5.8 Reaction Mechanism and Rate Law
5.7 Introduction to Reaction Mechanisms
5.2 Introduction to Rate Law
A student investigates the kinetics of the reaction represented by the equation below at \(450\text{ K}\):
\[ \text{NO}_2\text{(g)} + \text{CO(g)} \rightarrow \text{NO(g)} + \text{CO}_2\text{(g)} \]
The student performs several trials at constant temperature and observes that doubling the initial concentration of \(\text{CO(g)}\) while keeping the initial concentration of \(\text{NO}_2\text{(g)}\) constant has no effect on the initial rate of the reaction. Which of the following statements best explains why \(\text{CO(g)}\) does not appear in the rate law for this reaction?
\[ \text{NO}_2\text{(g)} + \text{CO(g)} \rightarrow \text{NO(g)} + \text{CO}_2\text{(g)} \]
The student performs several trials at constant temperature and observes that doubling the initial concentration of \(\text{CO(g)}\) while keeping the initial concentration of \(\text{NO}_2\text{(g)}\) constant has no effect on the initial rate of the reaction. Which of the following statements best explains why \(\text{CO(g)}\) does not appear in the rate law for this reaction?
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