---
title: "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.  | 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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url: "https://nerd-notes.com/ubq/123721/"
date_modified: "2026-09-28T12:02:09+00:00"
---

# 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.

| 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?

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.

| 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?

- **A.** \(\text{Mixture 4} > \text{Mixture 1} > \text{Mixture 2} > \text{Mixture 3}\)
- **B.** \(\text{Mixture 2} > \text{Mixture 4} > \text{Mixture 3} > \text{Mixture 1}\)
- **C.** \(\text{Mixture 2} > \text{Mixture 3} > \text{Mixture 4} > \text{Mixture 1}\)
- **D.** \(\text{Mixture 3} > \text{Mixture 1} > \text{Mixture 2} > \text{Mixture 4}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123721/*