The enthalpy change $\left(\mathrm{\Delta H}\right)$ for the reaction. ${\mathrm{N}}_{2( \mathrm{g})}+3{\mathrm{H}}_{2 \mathrm{g})}\to 2{\mathrm{NH}}_{3( \mathrm{g})}$ is $-92.38 \mathrm{kJ}$ at $298 \mathrm{K}.$ The internal energy change $\mathrm{\Delta U}$ at $298 \mathrm{K}$ is: 

Assertion: Water in liquid state is more stable than ice at room temperature.

Reason: Water in liquid form has higher entropy than ice.

Assertion: For a reaction $2{\mathrm{NH}}_3\left(\mathrm{g}\right)⟶{\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right): \mathrm{\Delta H}>\mathrm{\Delta E}$ 

Reason: Enthalpy change is always greater than internal energy change.