Figure shows plot of pV/T versus p for 1.00 x${{10}^{-3}} kg of oxygen gas at two different temperatures.
<img src="/uploads/db3785/original/2X/f/f21db29b0bc5bc9c7b88d2b33e88b55293e6585d.png" width="317" height="184">
(i) What does the dotted plot signify?
(ii) Which is true T1 > T2 or T1 < t2 ?
(iii) What is the value of pV/T, where the curves meet onthey-axis?
(iv) If we obtained similar plots for 1.00 x {{10}^{-3}} kg of hydrogen, would we get the same value of pV/T at the point where the curves meet on the y-axis? If not, what mass of hydrogen yields the same value ofpV/T (for low pressure high temperature region of the plot)? (.Molecular mass of { H }*{ 2 } = 2.02 u,
{{O}*{2}}$ = 32.0 u, R = 8.31 Jmol-1K-1).

(i) Dotted plot shows that pV/T is a constant quantoty ( pV/T = mR) which is independent of pressure .It signifies the ideal gas behaviour.

(ii)As curve at temperature { T }_{ 1 } is closer to the dotted plot than the curve at temperature

{ T }_{ 2 }. Since, the behaviour of a real gas approaches the behaviour of perfect gas when temperature is increased, so’

{ T }_{ 1 } >

{ T }_{ 2 }.

(iii) The value of pV/T , where the curves meet on y-axis is equal to µR

Now, given mass of oxygen gas = 1.00 x {{10}^{-3}} kg = 1g