Enthalpy $(H)$ is equal to

$A$ perfect gas $(0.1 \ mol)$ having $\overline{C}_{v}=1.50 \ R$ (independent of temperature) undergoes the transformation shown in the graph from point $1$ to point $4$. If each step is reversible,the total work done $(w)$ while going from point $1$ to point $4$ is $(-)$ . . . . . . $J$ (nearest integer). [Given: $R=0.082 \ L \ atm \ K^{-1} \ mol^{-1}$,$1 \ L \ atm = 101.3 \ J$]

Observe the following properties:
$I$. Molar volume
$II$. Mass
$III$. Internal energy
$IV$. Volume
$V$. Enthalpy
$VI$. Temperature
$VII$. Density
The intensive properties in the above list are:

$A$ gas expands from a volume of $1 \ m^{3}$ to a volume of $2 \ m^{3}$ against an external pressure of $10^{5} \ Nm^{-2}$. The work done by the gas will be

Which of the following is an intensive property?

During an isothermal expansion of an ideal gas,its: