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. `0.256 JK^(-1) and T_(1) lt T(2)`
B. `8.314 mol^(-1) K^(-1) and T_(1) gt T(2)`
C. `0.256 JK^(-1) and T_(1) gt T(2)`
D. `4.28 JK^(-1) and T_(1) lt T(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 value of P.
That is why, ideally it is a straight line.
`:. (PV)/T = (1 gm)/(32 gm) xx 8.31 J "mole"^(-1) K^(-1)`
`= 0.256 JK^(-1)`. Also, `T_(1) gt T_(2)`.