The relation between change in internal energy $(\Delta E)$,change in enthalpy $(\Delta H)$,and work done $(W)$ is represented as:

An ideal gas is allowed to expand from $2 \ dm^3$ to $6 \times 10^{-3} \ m^3$ against a constant external pressure of $1 \ bar$. The work done in $kJ$ is (in $kJ$)

Work done during isothermal expansion of $1 \, \text{mole}$ of an ideal gas from $10 \, \text{atm}$ to $1 \, \text{atm}$ at $300 \, \text{K}$ is ....... $\text{cal}$ (Gas constant $R = 2 \, \text{cal} \, \text{K}^{-1} \, \text{mol}^{-1}$) (in $.8$)

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:

$2$ moles of an ideal gas expands isothermally from $5$ $dm^3$ to $10$ $dm^3$ at a constant external pressure of $1.5$ bar. Calculate the work done.

What is the enthalpy change (in $J$) for converting $9 \ g$ of $H_2O(l)$ at $+10^{\circ}C$ to $H_2O(l)$ at $+20^{\circ}C$? $(C_p(H_2O(l)) = 75 \ J \ mol^{-1} \ K^{-1})$