[Gunther1991]

Hey, so this is my fist post, but how would you go about doing this? Thanks.

The equation d/p = M/RT, which can be derived from the ideal gas equation suggests that the density (d), in grams per liter, divided by the pressure (p) should be a constant. (M is the molecular mass of the gas.) The following gas density data were obtained for O2 (g) at various pressures at 273.15 K.

p (mm Hg) 760.00
d (g/L) 1.428962

p (mm Hg) 570.00
d (g/L) 1.071485

p (mm Hg) 380.00
d (g/L) 0.714154

p (mm Hg) 190.00
d (g/L) 0.356985

a. Calculate values of d/p, and with a graph or by other means determine the ideal value of the term d/p for O2 (g) at 273.15 K. (The ideal value is the value associated with an ideal gas. Since an ideal gas is one in which intermolecular interactions are negligible, all gases become ideal in the limit of zero pressure.)

b. Use the value of d/p obtained in part a to calculate the precise value for the atomic mass of oxygen and compare this with the accepted value. Account for any differences.

[billnotgatez]

According to forum rules you must show your attempt at solving.

[Gunther1991]

Well, I plotted the values on a coordinate plane, in an attempt at solving, but I found the value at which P=0 to be a negative density.

[Borek]

Calculate values of d/p, and with a graph or by other means

Have you tried "other means"?

determine the ideal value of the term d/p for O2 (g) at 273.15 K. (The ideal value is the value associated with an ideal gas. Since an ideal gas is one in which intermolecular interactions are negligible, all gases become ideal in the limit of zero pressure.)

Is oxygen an ideal gas?