Calculating Mass of Air in an Ideal Gas Tire for Beginners

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To calculate the mass of air in an automobile tire with a volume of 0.6 m³ and a gage pressure of 200 kPa at 20 degrees Celsius, use the ideal gas equation PV = mRT/M. Convert the gage pressure to absolute pressure by adding atmospheric pressure, resulting in an absolute pressure of 214.7 kPa. Ensure the temperature is in Kelvin by converting 20 degrees Celsius to 293.15 K. With the known values for pressure (P), volume (V), temperature (T), and the molecular mass (M) of air, you can solve for the mass (m) of air in the tire. Correct unit conversions are essential for accurate calculations.
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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
 
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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.
 

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