For the reaction $C_{(s)} + O_{2_{(g)}} \rightarrow CO_{2_{(g)}}$,which of the following is true?

Calculate the change in internal energy $(\Delta U)$ if an ideal gas expands from $0.5 \text{ dm}^3$ to $3.5 \text{ dm}^3$ at a constant pressure of $2 \text{ bar}$ by absorbing $1800 \text{ J}$ of heat energy. (in $\text{ J}$)

An ideal gas,$\overline{C}_{V} = \frac{5}{2} R$,is expanded adiabatically against a constant pressure of $1 \ atm$ until it doubles in volume. If the initial temperature and pressure are $298 \ K$ and $5 \ atm$,respectively,then the final temperature is . . . . . . $K$ (nearest integer). [$\overline{C}_{V}$ is the molar heat capacity at constant volume]

Calculate the internal energy change of a system if the work done by the system is $8 \ J$ and the heat supplied to it is $40 \ J$. (in $J$)

For the gaseous reaction $A_{(g)} + 3B_{(g)} \rightarrow 3C_{(g)} + 3D_{(g)}$,the value of $\Delta U = 17 \, Kcal$ at $27 \, ^oC$. Assuming $R = 2 \, cal \, K^{-1} \, mol^{-1}$,the value of $\Delta H$ for the above reaction will be ....... $Kcal$.

Identify the reaction for which $\Delta H \neq \Delta E$ :