Predict the change in internal energy for an isolated system at constant volume.

The enthalpy change $(\Delta H)$ for the reaction,$N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$ is $-92.38 \ kJ$ at $298 \ K$. The internal energy change $\Delta U$ at $298 \ K$ is .............. $kJ$

Identify the correct equation relating enthalpy $(H)$ and internal energy $(E)$.

If the work done by $2 \ mol$ of an ideal gas during isothermal reversible expansion from $5 \ L$ to $50 \ L$ is $-189.1 \ L \ atm$,the temperature of the gas (in $^{\circ}C$) is

Assume each reaction is carried out in an open container. For which reaction will $\Delta H = \Delta E$ ?

Assertion : Absolute values of internal energy of substances cannot be determined.
Reason : It is impossible to determine exact values of constituent energies of the substances.