Work done in vaporisation of one mole of water at $373 \ K$ and the pressure of $1 \ atm$ is approximately (for ideal gas)......$J$

$A$ gas can be taken from state $A$ to state $B$ via two different paths $ACB$ and $ADB$. When path $ACB$ is used, $60 \text{ J}$ of heat flows into the system and $30 \text{ J}$ of work is done by the system. If path $ADB$ is used, the work done by the system is $10 \text{ J}$. The heat flow into the system in path $ADB$ is: (in $text{ J}$)

$C_2H_5OH(l) + 3O_2(g) \rightarrow 2CO_2(g) + 3H_2O(l)$. The enthalpy change $(\Delta H)$ for the above reaction at $27^{\circ}C$ is $-1366.5 \text{ kJ mol}^{-1}$. Calculate the internal energy change $(\Delta U)$ for the same reaction at this temperature.

For the reaction $CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}$,which of the following is true?

For the reaction $PCl_{5(g)} \to PCl_{3(g)} + Cl_{2(g)}$,which of the following relations is correct?

Calculate $\Delta U$ if $2 \ kJ$ heat is released and $10 \ kJ$ of work is done on the system. (in $kJ$)