Which of the following is the correct expression of the first law of thermodynamics for an isothermal process?

In a particular reaction, $4 \text{ kJ}$ of heat is released by the system and $12 \text{ kJ}$ of work is done on the system. Calculate the $\Delta H$ and $\Delta U$.

Calculate the change in enthalpy in a chemical reaction when work done is $-800 \ J$ and increase in internal energy is $600 \ J$. (in $J$)

Internal energy of an ideal gas increases in:

Which of the following is not equal to zero in a cyclic process?

For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$ at $298 \ K$,the enthalpy change $(\Delta H)$ is $-92.38 \ kJ$. What will be the internal energy change $(\Delta U)$ at $298 \ K$ in $kJ$?