AP Chemistry
5.2 Introduction to Rate Law
The kinetics of the gas-phase reaction represented below is investigated at \(298\text{ K}\):
\[ 2\,\text{NO(g)} + \text{O}_2\text{(g)} \rightarrow 2\,\text{NO}_2\text{(g)} \]
The experimentally determined differential rate law for the reaction is:
\[ \text{Rate} = k[\text{NO}]^2[\text{O}_2] \]
Four separate reaction mixtures are prepared at \(298\text{ K}\) by injecting specified amounts of each reactant into sealed, rigid vessels of different volumes, as shown in the table below.
Which of the following correctly ranks the four mixtures in order of their initial instantaneous reaction rate, from greatest to least?
\[ 2\,\text{NO(g)} + \text{O}_2\text{(g)} \rightarrow 2\,\text{NO}_2\text{(g)} \]
The experimentally determined differential rate law for the reaction is:
\[ \text{Rate} = k[\text{NO}]^2[\text{O}_2] \]
Four separate reaction mixtures are prepared at \(298\text{ K}\) by injecting specified amounts of each reactant into sealed, rigid vessels of different volumes, as shown in the table below.
| Mixture | Initial moles of \(\text{NO}\) (mol) | Initial moles of \(\text{O}_2\) (mol) | Vessel volume (L) |
|---|---|---|---|
| 1 | \(0.30\) | \(0.40\) | \(2.0\) |
| 2 | \(0.40\) | \(0.10\) | \(1.0\) |
| 3 | \(0.20\) | \(0.30\) | \(1.0\) |
| 4 | \(0.60\) | \(0.20\) | \(2.0\) |
Which of the following correctly ranks the four mixtures in order of their initial instantaneous reaction rate, from greatest to least?
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