Exothermic reactions occur in which of the following processes?

For a change in state of $1 \, \text{mole}$ of a non-ideal gas,the change in internal energy is $\Delta U = 30.0 \, \text{L} \cdot \text{atm}$. The state changes from $(2.0 \, \text{atm}, 3.0 \, \text{L}, 95 \, \text{K})$ to $(4.0 \, \text{atm}, 5.0 \, \text{L}, 245 \, \text{K})$. What is the change in enthalpy $(\Delta H)$ in $\text{L} \cdot \text{atm}$?

At $61 \ K$, one mole of an ideal gas of $1.0 \ L$ volume expands isothermally and reversibly to a final volume of $10.0 \ L$. What is the work done in the expansion (in $L \ atm$)?

For the reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$,the relationship between $\Delta H$ and $\Delta U$ is:

For $1 \, \text{mole}$ of an ideal gas,isothermal expansion occurs from a volume of $2 \, L$ to $6 \, L$ at a temperature of $300 \, K$. The value of $\Delta U$ for this process is .............

If $5 \ L$ of an ideal gas at a constant external pressure of $2 \ atm$ expands isothermally to a final volume of '$X$' $L$,the system does a work of $-2,026.4 \ J$. '$X$' (in $L$) is $(1 \ L \cdot atm = 101.32 \ J)$