Please help! I have a lab report on the following data and I cant seem to figure

Question

Please help! I have a lab report on the following data and I cant seem to figure it out. Using the data I collected below ( done using a gas apparatus at a constant temperature of 73 degrees F) , I have to calculate the theoretical and experimental moles(n) of the gas. The gas that we were working with was simply air and it was given to us that the gas constant for air is Ra=286.9 J/kg K. It also tals about how the molecular weight for air is therefore R/Ra. I cant seem to figure out how to work this problem, as my calculations keep showing that n changes significantly for each trial when I use the equation PV=nRT. I thought n would be constant as both p and v vary, but this isnt the case. Please help, very confused. Thanks

Pressure (hPa) Volume (mL) 75 60 175 55 300 50 475 45 625 40 925 35 1175 30 1625 25 2200 20

Explanation / Answer

Firstly convert everything in SI units

Temperature from degree F to degree K

Take the value of R = 8.314 J/mol K

then use ideal gas gas law to solve the equation and get the value of n.

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