For a reaction to be spontaneous at all temperatures, the values of enthalpy change and entropy change should be

Find $\Delta n$ when 1 mol of each $\text{NH}_{3(g)}$ and $\text{HCl}_{(g)}$, reacts to form solid $\text{NH}_4\text{Cl}$.

$\text{C}_2\text{H}_5\text{OH}(l) + 3\text{O}_2(g) \rightarrow 2\text{CO}_2(g) + 3\text{H}_2\text{O}(l)$
The value of enthalpy change ($\Delta H$) for above reaction at $27\,^\circ\text{C}$ is $-1366.5$ kJ $\text{mol}^{-1}$. Then value of internal energy change for the same reaction at this temperature will be

Which of the following processes has $\Delta S$ negative?