[Cami_Fo]

The problem states: 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.)


My problem is comprehension of what this question is asking. I have found the value of d/p: it is 0.00188. And I understand that the first question wants to see a graph of some sort and I have done that also but I am confused on the first part where it asks to find the ideal value. Even though it says "all gases become ideal in the limit of zero pressure" I don't understand because if we take p and set it equal to zero the function is undefined, right? Please help.

  I chose the last value of d/p as the ideal value because it was the closest one to zero that you could get on these intervals. The value is exactly 0.0018788684. Is this the correct way to do this? Also, the next part of the question asks for the atomic mass of the element based on the ideal value found. I got 32.00736896 g. Is this the correct approach because I did it and it came out to be approximately the atomic wt of diatomic oxygen.

[Cami_Fo]

why is no one helping me?

[UG]

How does your graph look like? What are on the axes?

[fledarmus]

Do you know how to graphically determine a limit?