- #1
gg_1
- 4
- 0
does anyone happen to know the density of compressed air?
What Is the Density of Compressed Air?
- Thread starter gg_1
- Start date
Click For Summary
Discussion Overview
The discussion centers around the density of compressed air, exploring how it can be calculated and the factors that influence it, including pressure and temperature. Participants reference both theoretical and practical aspects of determining air density under compression.
Discussion Character
- Exploratory, Technical explanation, Conceptual clarification
Main Points Raised
- One participant inquires about the density of compressed air.
- Another participant humorously suggests that the density can be arbitrary.
- A similar humorous response reiterates the previous point while suggesting a method to calculate density based on pressure.
- A participant provides a formula derived from the ideal gas law, noting its applicability under certain conditions (high temperatures and low pressures).
- A specific density value for dry air at 1 atm and 20 degrees Celsius is mentioned, approximately 1.20 kg/m³.
- One participant humorously states a density of 0.0 kg/m³, likely as a joke.
Areas of Agreement / Disagreement
The discussion contains multiple viewpoints, with no consensus on a single definition or method for calculating the density of compressed air. Some participants provide calculations while others offer humorous or non-standard responses.
Contextual Notes
The discussion references the ideal gas law and its limitations, particularly regarding temperature and pressure conditions. There is also a mention of a compressibility chart, indicating that the topic may involve more complex considerations than those presented.
Who May Find This Useful
This discussion may be of interest to individuals studying gas laws, thermodynamics, or those involved in practical applications of compressed air in engineering or physics.
- #2
minger
Science Advisor
- 1,494
- 2
It's whatever I want it to be.
- #3
mgb_phys
Science Advisor
Homework Helper
- 7,906
- 15
minger said:
Start with the density of normal air then multiply by however many atmospheres of pressure it's under.
- #4
kandelabr
- 110
- 0
you should start with
pV = mRT, divide by (V R T), and you get
m/V = p/RT.
p - pressure [Pa], V - volume [m3], m - mass [kg], R - gas constant (287 kJ/kg), T - temperature [K]
note that this is for ideal gas and so only accurate for high temperatures (room) and low pressures (up to 40, 50 bar).
check out this page: http://en.wikipedia.org/wiki/Compressibility_chart
pV = mRT, divide by (V R T), and you get
m/V = p/RT.
p - pressure [Pa], V - volume [m3], m - mass [kg], R - gas constant (287 kJ/kg), T - temperature [K]
note that this is for ideal gas and so only accurate for high temperatures (room) and low pressures (up to 40, 50 bar).
check out this page: http://en.wikipedia.org/wiki/Compressibility_chart
- #5
Bob S
- 4,662
- 8
For 1 atm (760 mm Hg, or ~100,000 Pa) dry air at 20 deg C, the density is about 1.20 kilograms per cubic meter.
- #6
Topher925
- 1,563
- 7
>0.0 kg/m3
Similar threads
- · Replies 22 ·
- · Replies 14 ·
- · Replies 5 ·
- · Replies 7 ·
- · Replies 8 ·
- · Replies 1 ·
- · Replies 7 ·
- · Replies 45 ·
- · Replies 2 ·