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 $, J$)?

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:

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

Consider the reaction at $298 \ K$:
$H_{2(g)} + Cl_{2(g)} \to 2HCl_{(g)}, \Delta H^o = -185 \ kJ$
What is $\Delta U^o$ for this reaction? .....$kJ$

$A$ gas occupies a volume of $2 \ L$ at $S.T.P.$ It absorbs $300 \ J$ of heat. If the pressure is $1 \ atm$,the volume becomes $2.5 \ L$. The change in internal energy $(\Delta U)$ for the process in $Joule$ is:

$A$ gas is allowed to expand in an insulated container against a constant external pressure of $2.5 \ atm$ from $2.5 \ L$ to $4.5 \ L$. The change in internal energy of the gas in joules is: (in $J$)