Chemistry Question: What is the mass of air?

The air is 20% oxygen and 80% nitrogen. What is the mass of air in a tire Car of 19.7 L and the internal pressure of 46.7 psi at 24 ° C? (That pressure is the same difference of 32 PSI is usually measured as the tire pressure 32 psi + 14.7 psi. You have to use a weighted average of the molar mass of air.)

I begin with the ideal gas law: PV = nRT n Solving the equation is: n = PV / RT're given the pressure as: 46.7 lb / in ^ 2 and temperature: 24C = 297K is expressed in volume: 19.7L Now, all you need to do to solve n (moles of gas) to do some unit conversions of the gas constant. Then you have to determine an average molecular weight of the gas mixture: MW = 0.2 (MWO2) + 0.8 (MW N2) Multiply the value of N (moles of gas) times the average molecular weight of gas (g / mol) for the air mass in grams. I'm sure you can understand units and conversions to complete its own task.

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