The work done by a system is $8 \ J$,when $40 \ J$ heat is supplied to it. What is the increase in internal energy of the system in $J$?

One mole of an ideal gas at $27^oC$ is allowed to expand reversibly and adiabatically. If the work done by the system is $3 \, kJ$,then the final temperature of the gas will be ......$K$. (Given: $C_v = 20 \, J/K \cdot mol$)

Standard enthalpy of vaporisation $\Delta_{vap}H^o$ for water at $100\ ^oC$ is $40.66\ kJ\ mol^{-1}.$ The internal energy of vaporisation of water at $100\ ^oC$ (in $kJ\ mol^{-1}$) is ............... $kJ\ mol^{-1}$ (Assume water vapour to behave like an ideal gas)

$A$ gas occupies $1.5 \ L$ at $S.T.P.$ It is provided with $300 \ J$ of heat so that its volume becomes $2 \ L$ at a pressure of $1 \ atm$. The value of $\Delta U$ for the process is.....joule.

In the complete combustion of butanol $C_4H_9OH_{(l)}$,if $\Delta H$ is the enthalpy of combustion and $\Delta E$ is the heat of combustion at constant volume,then

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: