Considering entropy $(S)$ as a thermodynamic parameter,the criterion for the spontaneity of any process is

Given the entropy of $H_2$ and $HBr$ are $130.6 \, JK^{-1}$ and $198.5 \, JK^{-1}$ respectively,calculate the entropy of $Br_{2(g)}$ in the reaction $H_{2(g)} + Br_{2(g)} \rightarrow 2HBr_{(g)}$ where $\Delta S^{o} = 20.1 \, JK^{-1}$.

What is the entropy of vaporisation of water at $100\,^{\circ}C$,if the molar heat of vaporisation is $9710\,cal/mol$?

The process with negative entropy change is

Amongst the chemical reactions given below, the reactions with increasing entropy are
$(i)$ $H_2O_{(l)} \rightarrow H_2O_{(g)}$
$(ii)$ $C_{(s)} + CO_{2(g)} \rightarrow 2CO_{(g)}$
$(iii)$ $2H_{2(g)} + O_{2(g)} \rightarrow 2H_2O_{(l)}$
$(iv)$ $N_{2(g)} + O_{2(g)} \rightarrow \text{Mixture of } N_2 \text{ and } O_2$

Given $\Delta S_{Total} = -40 \ kJ/mol \cdot K$,$\Delta H_{System} = 2000 \ kJ/mol$,and $T = 400 \ K$. Find the value of $\Delta S_{System}$ in $kJ/mol \cdot K$.