Calculate the entropy change of the surrounding if $2 \ moles$ of $H_2$ and $1 \ mole$ of $O_2$ gas combine to form $2 \ moles$ of liquid water by releasing $525 \ kJ$ of heat to the surrounding at constant pressure and at $300 \ K$. (in $J \ K^{-1}$)

For the transformation $C(\text{graphite}) \rightarrow C(\text{diamond})$,$\Delta S$ is .......

Give the mathematical equation for entropy change.

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 $-1648 \times 10^3 \ J \ mol^{-1}$)

What is entropy? Explain its role in spontaneity.

The value of $\Delta S$ for freezing of $10 \ g$ of $H_2O_{(l)}$ (enthalpy of fusion is $80 \ cal/g$) at $0 \ ^\circ C$ and $1 \ atm$ pressure is.......$J/K$