I copied this from google. Read the next to last paragraph carefully.
Patrick Donovan
, former Student and Avid Procrastinator
Answered April 11, 2017
Luckily, under standard temperature and pressure, one mole of gaseous molecules occupies approximately 22.3 litres of space. This means that we can apply the ideal gas law to solve for the number of moles of substance: n=PV/RT. With the number of molecules, we can then find the mass of our sample. Inversely, we can solve for our pressure; P=nRT/V.
But no, there is no relationship between mass and pressure, without knowing the volume, moles, temperature, and molar mass.
If there's anything else I can help with, feel free to message.
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How do you graph the pressure of air and mass of air when given values? What is the y axis?
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