A sample of O2 gas is placed in a sealed 1.00 L flask and pressure is measured as temperature is changed. The data are plotted and the slope of the resulting line is equal to 0.00300 atm/K. The line passes through the origin of the graph. There are ???? g of O2 gas in the flask.

Answer 1

Since PV = nRT,
P/T (your slope)= nR/V = 0.0300 atm/K

n (the number of moles) = (V/R)*(P/T)
= (1 liter/0.08206 liter atm/mole K)* 0.003 atm K = 0.03656 moles

Convert that to grams

Answer 2

Here is how you convert it to grams

(0.03656 moles of O2)*[(32.0g of O2)/(1 mole of O2)]= ____g of O2