The correct relationship is

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

The enthalpy of vaporization of water at $100 \, ^\circ C$ is $40.63 \, kJ \, mol^{-1}$. The value of $\Delta U$ for this process is ....... $kJ \, mol^{-1}$.

$A$ mixture of $2 \ mol$ of carbon monoxide and $1 \ mol$ of oxygen in a closed vessel is ignited to convert the carbon monoxide to carbon dioxide. If $\Delta H$ is the enthalpy change and $\Delta E$ is the change in internal energy,then:

$5 \, mol$ of an ideal gas expands isothermally and irreversibly from a pressure of $10 \, atm$ to $1 \, atm$ against a constant external pressure of $1 \, atm$. The work done $(w_{irr})$ at $300 \, K$ is:

Identify the reaction for which $\Delta H \neq \Delta E$ :