According to the first law of thermodynamics,which of the following is correct? (Where $q =$ heat supplied to the system and $W =$ work done by the system)

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 is the value of $\Delta U$ in $kJ$ at $298 \ K$?

$A$ gas expands from a volume of $1 \text{ dm}^3$ to $1.25 \text{ dm}^3$ against a constant external pressure of $1 \text{ bar}$. Calculate the change in internal energy $(\Delta U)$ if $150 \text{ J}$ of heat is supplied to the system. (in $\text{ J}$)

For the gaseous reaction,$N_2O_4(g) \to 2NO_2(g)$,which of the following relations is correct?

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

“The mass and energy both are conserved in an isolated system”,is the statement of