For which of the following processes is $q = \Delta U$?

For which of the following reactions is $\Delta H \neq \Delta U$?

The heat change for the following reaction at $298 \ K$ and at constant pressure is $+7.3 \ kcal$: $A_2B_{(s)} \to 2A_{(s)} + 1/2B_{2(g)}$,$\Delta H = +7.3 \ kcal$. The heat change at constant volume would be:

In the reaction $H_2O_{(l)} \rightarrow H_2O_{(s)}$ at $0^{\circ}C$ and $1 \ atm$, the internal energy change is $-41 \ kJ / mol$. What will be the value of molar enthalpy change?

Assertion : For a reaction $2NH_{3(g)} \to N_{2(g)} + 3H_{2(g)}$ ; $\Delta H > \Delta E$.
Reason : Enthalpy change is always greater than internal energy change.

If $3 \ mol$ of an ideal gas at $300 \ K$ expand isothermally from $30 \ dm^3$ to $45 \ dm^3$ against a constant opposing pressure of $80 \ kPa$,then the amount of heat transferred is . . . . . . $J$.