Which is not the correct relation between enthalpy $(\Delta H)$ and internal energy $(\Delta E)$?

Two mole of an ideal gas is expanded isothermally and reversibly from $1 \ L$ to $10 \ L$ at $300 \ K$. The enthalpy change (in $kJ$) for the process is .....$kJ$

What is the constant external pressure of an ideal gas when expanded from $2 \times 10^{-2} \ m^3$ to $3 \times 10^{-2} \ m^3$,if the work done by the gas is $-5.09 \ kJ$?

Which one of the following is an extensive property?

For the reaction,$C_3H_{8(g)} + 5O_{2(g)} \longrightarrow 3CO_{2(g)} + 4H_2O_{(l)}$ at constant temperature,$\Delta H - \Delta U$ is:

Fill in the blanks:
$(i)$ The process of attaining thermal equilibrium between any two heat-conducting bodies is called the $\dots\dots$ law of thermodynamics.
$(ii)$ The law of thermodynamics is actually the law of $\dots\dots$.
$(iii)$ $A$ thermometer measures temperature according to the $\dots\dots$ law of thermodynamics.