If $100 \ L$ of an ideal gas at a pressure of $2 \ atm$ is compressed isothermally and reversibly to a final volume of '$X$' $L$ and releases $460.6 \ L \ atm$ of heat,the final volume '$X$' (in $L$) is

In a process,$701 \, J$ of heat is absorbed by a system and $394 \, J$ of work is done by the system. What is the change in internal energy for the process (in $, J$)?

$A$ gas absorbs $150 \ J$ of heat and expands by $300 \ cm^3$ against a constant external pressure of $2 \times 10^5 \ N \ m^{-2}$. What is the change in internal energy $(\Delta U)$ of the system (in $J$)?

$A$ gas undergoes a change from state $A$ to state $B$. In this process,the heat absorbed and work done by the gas are $5\, J$ and $8\, J$,respectively. Now,the gas is brought back to $A$ by another process during which $3\, J$ of heat is evolved. In this reverse process of $B$ to $A$:

For a gaseous reaction,$A_{(g)} + 3B_{(g)} \to 3C_{(g)} + 3D_{(g)}$. The value of $\Delta E$ is $17 \ kcal$ at $27 \ ^oC$. The value of $\Delta H$ in $kcal$ will be:

The relation between $\Delta H$ and $\Delta U$ for the reaction $2 SO_{3(g)} \longrightarrow 2 SO_{2(g)} + O_{2(g)}$ is: