The enthalpy of vapour is $10 \ kcal/mole$ higher than liquid at $350 \ K$ and $2 \ atm$. Under given conditions,the difference in internal energy of vapour and liquid will be $...... \ cal$.

Which of the following relations is correct for the internal energy change $(\Delta U)$ in a process occurring at constant volume?

$A$ mixture of $2 \ mol$ of $CO_{(g)}$ and $1 \ mol$ of $O_{2(g)}$ is ignited to convert $CO$ to $CO_2$. Which of the following relations is correct?

Based on the first law of thermodynamics,which one of the following is correct?

Find the approximate value of $(\Delta H - \Delta U)$ in $J \cdot mol^{-1}$,for the formation of $CO$ from its elements at $298 \ K$. $(R = 8.314 \ J \cdot K^{-1} \ mol^{-1})$

$A$ 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 $A$: