Calculating Mass of Air in an Ideal Gas Tire for Beginners

  • Thread starter Thread starter johnleno007
  • Start date Start date
  • Tags Tags
    Gas Ideal gas
Click For Summary
SUMMARY

The discussion focuses on calculating the mass of air in an automobile tire using the ideal gas law. Given a tire volume of 0.6 m3, a gauge pressure of 200 kPa, and a temperature of 20 degrees Celsius, the ideal gas equation PV = mRT/M is applied. The absolute pressure must be calculated by adding atmospheric pressure (approximately 100 kPa) to the gauge pressure. The molecular mass of air is also required for the calculation.

PREREQUISITES
  • Understanding of the ideal gas law (PV = nRT)
  • Knowledge of pressure units (gauge vs. absolute pressure)
  • Ability to convert temperature from Celsius to Kelvin
  • Familiarity with molecular mass of air (approximately 29 g/mol)
NEXT STEPS
  • Learn how to convert gauge pressure to absolute pressure in practical applications
  • Study the ideal gas law in detail, including its derivation and applications
  • Explore unit conversion techniques, particularly for pressure and temperature
  • Investigate the properties of gases, focusing on the molecular mass of various gases
USEFUL FOR

Students in physics or engineering, automotive technicians, and anyone interested in thermodynamics and gas laws.

johnleno007
Messages
1
Reaction score
0
I have no clue how to start this problem can someone help?

Problem: An automobile tire that has V= 0.6 m3 is inflated to a gage pressure of 200 kPA. Calculate the mass of air in the tire if the temperature is 20 Degree Celsius.

Suggestion from my teacher: Air is assumed to be an ideal gas. Use the ideal gas equation (Absolute pressure and absolute temperature (Kelvin). PAtm= 14.7 #/in V= 100 kPA.

Please help
 
Physics news on Phys.org
johnleno007 said:
I have no clue how to start this problem can someone help?

Problem: An automobile tire that has V= 0.6 m3 is inflated to a gage pressure of 200 kPA. Calculate the mass of air in the tire if the temperature is 20 Degree Celsius.

Suggestion from my teacher: Air is assumed to be an ideal gas. Use the ideal gas equation (Absolute pressure and absolute temperature (Kelvin). PAtm= 14.7 #/in V= 100 kPA.

Please help

PV = mRT/M

You know the pressure (P), the volume (V), the temperature (T) and can easily obtain the molecular mass (M) of air. You can solve for m.

Make sure that you use the correct units for everything.
 

Similar threads

Chemistry Ideal Gas Law and Partial Pressures
  • · Replies 16 ·
Replies
16
Views
3K
Chemistry How does it work to mix two gases reversibly in this device?
  • · Replies 1 ·
Replies
1
Views
2K
Calculating Mercury Column Height in J-Shaped Tube: Manometry Homework Solution
  • · Replies 7 ·
Replies
7
Views
2K
Calculating enthalpies of gas mixtures
  • · Replies 3 ·
Replies
3
Views
2K
Why must we use absolute temperature for the Ideal Gas Law?
  • · Replies 10 ·
Replies
10
Views
3K
Undergrad How to calculate the mass of gas in a tank?
  • · Replies 109 ·
4
Replies
109
Views
8K
Ideal Gas Law: What is the new pressure based on factors?
  • · Replies 18 ·
Replies
18
Views
2K
An ideal gas closed system reversible process
  • · Replies 2 ·
Replies
2
Views
3K
Thermodynamic Problem: Ideal Gas Expansion and Work Calculation
  • · Replies 16 ·
Replies
16
Views
2K
Calculating ΔE Difference for 2 Samples of Monatomic Ideal Gas
  • · Replies 4 ·
Replies
4
Views
2K