Which amongst the following options is the correct relation between change in enthalpy and change in internal energy?

Work done during isothermal expansion of $1 \, \text{mole}$ of an ideal gas from $10 \, \text{atm}$ to $1 \, \text{atm}$ at $300 \, \text{K}$ is ....... $\text{cal}$ (Gas constant $R = 2 \, \text{cal} \, \text{K}^{-1} \, \text{mol}^{-1}$) (in $.8$)

Which law of thermodynamics can be considered as the definition of temperature?

On what factors does the enthalpy of dilution of a solution depend?

Enthalpy change for freezing of $1 \ g$ of water at $1 \ bar$ and $0^{\circ} C$ is $334 \ J$. Calculate the internal energy change in $J$ when $1 \ g$ of water is converted into ice?

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