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 $J$)?

When a certain volume of gas expands against a constant external pressure of $2.40 \times 10^5 \ Pa$ at $300 \ K$ to a final volume of $2.2 \times 10^{-3} \ m^3$. If the work obtained is $-0.048 \ kJ$,what is the initial volume of the gas?

For the gaseous reaction $A_{(g)} + 3B_{(g)} \rightarrow 3C_{(g)} + 3D_{(g)}$,the value of $\Delta U = 17 \, Kcal$ at $27 \, ^oC$. Assuming $R = 2 \, cal \, K^{-1} \, mol^{-1}$,the value of $\Delta H$ for the above reaction will be ....... $Kcal$.

If the internal energy of an ideal gas decreases by the same amount of the work done by the system,the process is

Mark the correct statement.

Identify from the following reactions the one that exhibits negative work done by the system.