Fig shows of `PV//T` versus P for `1.00 xx 10^(-3) kg` of oxygen gas at two different temperatures.
(a) What does the dotted plot signify ?
(b) Which is true : `T_(1) lt T_(2) or T_(2) lt T_(1) ?`
( c) What is the value of `PV//T` where the curves meet on the Y-axis ?
(d) If we obtained similar plot for `1.00 xx 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 yield the same value of `PV//T` (for low pressure high temperature region of the plot) ? (Molecular mass of `H = 2.02 u`, of `O = 32.0 u, R = 8.31 J "mol"^(-1) K^(-1)`

Explanation

(i) For the dotted line, `(PV)/(T)=` constant.
It represents the behaviour of an ideal gas
(ii) The gas equation PV=RT is true only at high temperature.
In figure, curve for `T_(1)` is coloser to the dotted line than curve for `T_(2)` Hence the relation between `T_(1)` and `T_(2)` is `T_(1)gtT_(2)`
(iii) `(PV)/(T)=muR` , Here `mu=(m)/(M)=(2)/(32)=(1)/(16)`
`therefore (PV)/(T)=(1)/(16)xx8.31=0.519 J//K`