Given is the graph between `(PV)/T` and P for 1 gm of oxygen gas at two different temperatures `T_(1) and T_(2)` Fig. Given, density of oxygen `= 1.427 kg m^(-3)`. The value of `(PV)//(T)` at the point A and the relation between `T_(1) and T_(2)` are respectively :

Options

A. `0.259JK^(-1)andT_(1)ltT_(2)`
B. `8.314Jmol^(-1)K^(-1)andT_(1)gtT_(2)`
C. `0.259JK^(-1)andT_(1)gtT_(2)`
D. `4.28JK^(-1)andT_(1)ltT_(2)`

Answer

C

Explanation

`PV=nRT=(m)/(M)RT`
Where m = mass of the gas and `(m)/(M)=n` = number of moles.
`(PV)/(T)=nR` = a constant for all values of P.
That is why, ideally it is a straight line.
`therefore (PV)/(T)=(1g)/(32gmol^(-1))xx8.31Jmol^(-1)K^(-1)=0.259JK^(-1)`
Also `T_(1)gtT_(2)` (Due to intermolecular attraction volume will be lesser at lower temperature).