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title: "A sample containing \\(1.00 \\text{ mol}\\) of \\(\\text{N}_2\\text{(g)}\\) is held in a container at a constant temperature of \\(273 \\text{ K}\\). A student measures the pressure and volume of the gas sample across four different trials and calculates the ratio \\(\\dfrac{PV}{nRT}\\), as summarized in the table below.  | Trial | Pressure (\\(\\text{atm}\\)) | \\(\\dfrac{PV}{nRT}\\) | |—|—|—| | 1 | \\(1.0\\) | \\(1.00\\) | | 2 | \\(100\\) | \\(0.87\\) | | 3 | \\(300\\) | \\(1.00\\) | | 4 | \\(800\\) | \\(1.52\\) |  Based on the data in the table, which of the following best explains why \\(\\dfrac{PV}{nRT} > 1.00\\) in trial 4?"
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date_modified: "2026-08-21T06:53:49+00:00"
---

# A sample containing \(1.00 \text{ mol}\) of \(\text{N}_2\text{(g)}\) is held in a container at a constant temperature of \(273 \text{ K}\). A student measures the pressure and volume of the gas sample across four different trials and calculates the ratio \(\dfrac{PV}{nRT}\), as summarized in the table below.

| Trial | Pressure (\(\text{atm}\)) | \(\dfrac{PV}{nRT}\) |
|—|—|—|
| 1 | \(1.0\) | \(1.00\) |
| 2 | \(100\) | \(0.87\) |
| 3 | \(300\) | \(1.00\) |
| 4 | \(800\) | \(1.52\) |

Based on the data in the table, which of the following best explains why \(\dfrac{PV}{nRT} > 1.00\) in trial 4?

A sample containing \(1.00 \text{ mol}\) of \(\text{N}_2\text{(g)}\) is held in a container at a constant temperature of \(273 \text{ K}\). A student measures the pressure and volume of the gas sample across four different trials and calculates the ratio \(\dfrac{PV}{nRT}\), as summarized in the table below.

| Trial | Pressure (\(\text{atm}\)) | \(\dfrac{PV}{nRT}\) |
|---|---|---|
| 1 | \(1.0\) | \(1.00\) |
| 2 | \(100\) | \(0.87\) |
| 3 | \(300\) | \(1.00\) |
| 4 | \(800\) | \(1.52\) |

Based on the data in the table, which of the following best explains why \(\dfrac{PV}{nRT} > 1.00\) in trial 4?

- **A.** The volume occupied by the gas molecules themselves is no longer negligible relative to the total container volume, resulting in an actual volume that is greater than predicted by the ideal gas law.
- **B.** The intermolecular attractive forces between the \(\text{N}_2\) molecules become dominant, resulting in an actual pressure that is greater than predicted by the ideal gas law.
- **C.** The average kinetic energy of the \(\text{N}_2\) molecules increases due to the high collision frequency at extreme pressure, resulting in an increase in gas temperature.
- **D.** The \(\text{N}_2\) molecules undergo dissociation into individual \(\text{N}\) atoms at high pressure, resulting in a greater number of moles than the initial \(1.00 \text{ mol}\).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119565/*