What is the internal energy change when $62 \ J$ of work is done on the system and $128 \ J$ of heat is transferred to the surrounding (in $J$)?

For the reaction $C_2H_5OH_{(l)} + 3O_{2(g)} \rightarrow 2CO_{2(g)} + 3H_2O_{(l)}$,the enthalpy change $(\Delta H)$ at $27\,^oC$ is $-1366.5 \,kJ\,mol^{-1}$. What will be the value of the internal energy change $(\Delta U)$ in $kJ\,mol^{-1}$ at the same temperature?

The work done by the system is $8 \, J$. When $40 \, J$ of heat is supplied to the system,the change in internal energy of the system during the process is ...... $J$.

$\Delta_{vap} H^{\ominus}$ for water is $+40.49 \ kJ \ mol^{-1}$ at $1 \ bar$ and $100^{\circ} C$. The change in internal energy for this vaporization under the same conditions is . . . . . . . . . . $kJ \ mol^{-1}$. (Integer answer) (Given $R = 8.3 \ J \ K^{-1} \ mol^{-1}$)

In an adiabatic expansion of an ideal gas,which of the following relations holds true?

If the internal energy of an ideal gas decreases by the same amount of the work done by the system,the process is