For the reaction,

$$2 \mathrm{H}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}, \Delta \mathrm{H}^{\circ}=-573.2 \mathrm{~kJ}$$

What is heat of decomposition of water per mol?

For the reaction,

$$\mathrm{C}_3 \mathrm{H}_{8(\mathrm{~g})}+5 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 3 \mathrm{CO}_{2(\mathrm{~g})}+4 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}$$

at constant temperature, $\Delta \mathrm{H}-\Delta \mathrm{U}$ is

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

Two moles of an ideal gas is expanded isothermally from a volume of $300 \mathrm{~cm}^3$ to 2.5 $\mathrm{dm}^3$ at 298 K against a constant pressure at 1.9 bar. Calculate the work done in joules.