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)`

Options

A. (i) only
B. (i) and (ii) only
C. All of the above
D. None of the above

Answer

C

Explanation

(The dotted line in the diagram shows that there is no deviation in the value of `(pV)/(nT)` for different temperatures `T_(1)` and `T_(2)` for increasing pressure so, this gas behaaves ideally. Hence, dotted line corresponds to 'ideal gas' behaviour.
(ii) At high temperature, the deviation of the gas is less and at low temperature the deviation of gas is more. In the graph,deviation fof `T_(2)` is greater than for`T_(1)` Thus
`T_(1)gtT_(2)`
(iii) Since, the two curves intersect at dotted line so, the value of `(pV)/(nt)` at that point on the y-axis is same for all gases.