Nitrogen Pressure-Temperature Calculator
Here’s a comprehensive table that provides key information on the relationship between pressure and temperature for nitrogen, as well as the physical and chemical properties of nitrogen that affect its behavior in various industrial and scientific applications.
Nitrogen Pressure-Temperature Table and Key Information
| Property | Details |
|---|---|
| Molecular Formula | N₂ |
| Molar Mass | 28.0134 g/mol |
| Critical Temperature | -147°C (126 K) |
| Critical Pressure | 3.39 MPa (33.5 atm) |
| Boiling Point (1 atm) | -196°C (77 K) |
| Melting Point (1 atm) | -210°C (63 K) |
| Triple Point Temperature | -210°C (63.15 K) |
| Triple Point Pressure | 12.52 kPa |
| Density (Gas, 1 atm, 0°C) | 1.2506 kg/m³ |
| Density (Liquid, -195.8°C) | 808.5 kg/m³ |
| Specific Heat Capacity | 1.040 J/g°C (gas) |
| Thermal Conductivity | 0.02583 W/mK (at 27°C) |
Pressure-Temperature Relationship for Nitrogen (Ideal Gas Law)
For gases like nitrogen, the relationship between pressure, temperature, and volume is often described by the Ideal Gas Law:
PV=nRTPV = nRTPV=nRT
Where:
- PPP = Pressure (in Pascals or atm)
- VVV = Volume (in liters or cubic meters)
- nnn = Number of moles of gas
- RRR = Ideal gas constant (8.314 J/mol·K or 0.0821 L·atm/mol·K)
- TTT = Temperature (in Kelvin)
Nitrogen Gas Behavior at Different Conditions
| Temperature (K) | Pressure (atm) | Pressure (Pa) | Comments |
|---|---|---|---|
| 77 K | 1 atm | 101,325 Pa | Nitrogen becomes a liquid at this temperature (boiling point). |
| 126 K | 33.5 atm | 3.39 MPa | Critical temperature of nitrogen, beyond which it cannot be liquefied by pressure. |
| 200 K | 4.93 atm | 500,000 Pa | Nitrogen gas at low temperatures, slightly above boiling point, at moderate pressure. |
| 273 K (0°C) | 1 atm | 101,325 Pa | Standard conditions for nitrogen gas at room temperature and atmospheric pressure. |
| 300 K (27°C) | 1 atm | 101,325 Pa | Nitrogen gas under typical laboratory or room conditions. |
| 400 K | 1 atm | 101,325 Pa | Nitrogen gas expands significantly at higher temperatures. |
| 500 K | 1 atm | 101,325 Pa | Nitrogen under high-temperature conditions for industrial processes. |
Factors Affecting Nitrogen’s Pressure-Temperature Behavior
- Temperature:
- As the temperature increases, the kinetic energy of nitrogen molecules increases, causing them to move faster and exert more pressure on the walls of a container.
- At constant volume, the pressure of nitrogen increases linearly with temperature (Ideal Gas Law).
- Pressure:
- At low temperatures (below the critical point), nitrogen can condense into a liquid. The pressure required for this phase change depends on temperature.
- At high temperatures, nitrogen behaves increasingly like an ideal gas.
- Critical Point:
- The critical point of nitrogen is the temperature (126 K or -147°C) and pressure (33.5 atm or 3.39 MPa) beyond which nitrogen cannot be liquefied, no matter how much pressure is applied.
- Phase Transitions:
- Boiling Point: At 1 atm, nitrogen boils at -196°C (77 K), turning from liquid to gas. Below this temperature, nitrogen exists in a liquid state.
- Melting Point: Nitrogen solidifies at -210°C (63 K), transitioning from a liquid to a solid phase.
- Triple Point: At -210°C and 12.52 kPa, nitrogen can coexist in solid, liquid, and gaseous forms.
- Density and Volume:
- The density of nitrogen gas decreases as temperature increases. At higher temperatures and constant pressure, nitrogen expands, occupying more volume.
- Ideal Gas Assumptions:
- Nitrogen behaves as an ideal gas under standard conditions (room temperature and pressure). However, at very high pressures or very low temperatures, deviations from ideal behavior occur due to intermolecular forces.
Practical Applications of Nitrogen's Pressure-Temperature Relationship
- Cryogenics:
- Liquid nitrogen (at 77 K) is used in cryogenic applications such as preserving biological samples, cooling superconductors, and creating ultra-low-temperature environments.
- Pressurization in Aircraft and Industrial Systems:
- Nitrogen is used for pressurizing aircraft tires and hydraulic systems due to its inert nature and predictable pressure-temperature behavior.
- Welding and Metal Processing:
- Nitrogen is used as an inert gas in welding, and its behavior under high-temperature conditions is crucial for ensuring safe and effective welding environments.
- Cooling Systems:
- Gaseous nitrogen is used in industrial cooling systems and electronics cooling due to its low boiling point and high thermal stability.
- Gas Storage:
- In compressed gas storage, knowing the relationship between pressure and temperature helps in determining safe storage conditions for nitrogen gas cylinders.
Nitrogen Phase Diagram Summary
The phase diagram of nitrogen shows its solid, liquid, and gas states at different temperatures and pressures:
- Solid: Exists below the melting point (-210°C or 63 K) at low pressures.
- Liquid: Exists between the melting point and boiling point (-196°C or 77 K) at 1 atm.
- Gas: Exists above the boiling point at higher temperatures.
Understanding these transitions is critical for various industrial applications, particularly in cryogenics, where nitrogen is used to achieve and maintain extremely low temperatures.