Calculating Oxygen Mass and Leak in a Tank Using Ideal Gas Law

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SUMMARY

The discussion revolves around calculating the initial mass of oxygen and the mass that leaked from a tank using the Ideal Gas Law. The tank has a volume of 7.60 x 10^-2 m^3, filled with oxygen (molar mass 32.0 g/mol) at a gauge pressure of 3.25 x 10^5 Pa and a temperature of 36.0 degrees Celsius. The correct approach involves converting gauge pressure to absolute pressure by adding atmospheric pressure, which resolves the initial mass calculation error. The final mass of oxygen that leaked is determined after calculating the pressure at a lower temperature of 22.4 degrees Celsius, where the pressure is 1.80 x 10^5 Pa.

PREREQUISITES
  • Understanding of the Ideal Gas Law (pV = nRT)
  • Knowledge of pressure conversions (gauge to absolute pressure)
  • Familiarity with units of measurement (Pa, m^3, g/mol)
  • Basic thermodynamics concepts (temperature effects on gas behavior)
NEXT STEPS
  • Learn how to apply the Ideal Gas Law in various scenarios
  • Study pressure conversion techniques in gas calculations
  • Explore the effects of temperature on gas volume and pressure
  • Investigate methods for calculating gas leaks in pressurized systems
USEFUL FOR

Students in physics or engineering courses, professionals in welding and gas handling, and anyone involved in gas storage and leak detection methodologies.

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Homework Statement



A welder fills a tank, volume 7.60 x 10^-2 m^3, with oxgyen (32.0 g/mol) at gauge pressure 3.25 x 10^5 Pa and temp. 36.0 degrees C. The tank has a small leak, and some of the oxygen leaks. When temp. is 22.4 degrees C, pressure of oxygen in tank is 1.80 x 10^5 Pa.

Find initial mass of oxygen.
Find mass of oxygen that leaked out.


Homework Equations



pV = nRT

The Attempt at a Solution



I understand that I need to find the answer to the first part in order to get the answer to the second part. I used the ideal gas law equation to solve the first part and got the answer to be 308 grams but it keeps telling me that's wrong.
 
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Try converting the gauge pressure to absolute pressure by adding the atmospheric pressure to the gauge pressure.
 
thanks I tried that and got the correct answer :)
 

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