What is the change in internal energy of the system when the work done by the system is $150 \ J$ and the system releases $300 \ J$ of heat?

$A$ gas absorbs $150 \ J$ of heat and expands by $300 \ cm^3$ against a constant external pressure of $2 \times 10^5 \ N \ m^{-2}$. What is the change in internal energy $(\Delta U)$ of the system (in $J$)?

For the reaction $CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}$,which of the following is true?

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 $kJ$?

During the free expansion of an ideal gas in an isolated chamber,

What is the value of the increase in internal energy when a system does $8 \ J$ of work on the surroundings by supplying $40 \ J$ of heat to it (in $J$)?