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

#1

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).

#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 }\$.
(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