Figure shows plot of pV/T versus p for 1.00 x${{10}^{-3}}$ kg of oxygen gas at two different temperatures.

(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).

# Figure shows plot of pV/T versus p for 1.00 x${{10}^{-3}}$ kg

**prasanna**#1

**prasanna**#2

(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 }$ >*

${ T }{ 2 }$.

${ T }

(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