Identify the reaction/process in which the entropy decreases.

$\Delta S_{surr}$ for an exothermic reaction is

For the oxidation of iron:
$4 Fe_{(s)} + 3 O_{2(g)} \rightarrow 2 Fe_2O_{3(s)}$
The entropy change is $-549.4 \ J \ K^{-1} \ mol^{-1}$ at $298 \ K$. Despite the negative entropy change of this reaction,why is the reaction spontaneous?
($\Delta_r H^\Theta$ for this reaction is $-1648 \times 10^3 \ J \ mol^{-1}$)

If the enthalpy change for the transition of liquid water to steam is $30 \ kJ \ mol^{-1}$ at $27 \ ^oC,$ the entropy change for the process would be ............. $J \ mol^{-1} \ K^{-1}$

What is the melting point of benzene if $\Delta H_{fusion} = 9.95 \ kJ/mol$ and $\Delta S_{fusion} = 35.7 \ J/K \cdot mol$?

Calculate the entropy change when $1 \, \text{mole}$ of ice is converted into water at $0 \, ^\circ\text{C}$. (The enthalpy change for the conversion of ice to liquid at $0 \, ^\circ\text{C}$ is $6.0 \, \text{kJ} \, \text{mol}^{-1}$).