For which of the following reactions is $\Delta U = \Delta H$?

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 $\text{L} \cdot \text{atm}$?

Any series of operations so carried out that at the end,the system is back to its initial state is called:

Calculate the work done in the oxidation of one mole $HCl_{(g)}$ at $27^{\circ} C$,according to the reaction: $4 HCl_{(g)} + O_{2_{(g)}} \rightarrow 2 Cl_{2_{(g)}} + 2 H_{2}O_{(g)}$ $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$ (in $J$)

Conditions of standard state used in thermochemistry is

What is the internal energy change when $2$ moles of an ideal gas at $25^{\circ} C$ is compressed isothermally and reversibly from $1.0 \ bar$ to $10.0 \ bar$?