Consider the following process (each step involves a reversible change) 

Considering the ideal gas behavior of  $H_2$ gas, Select the correct choice(s): 

A)  $\Delta S_{X\to Z}=\frac{q}{T}=0$ (reversible adiabatic change)
B)  $\Delta S_{X\to Z\to Y}=\Delta S_{X\to Y}=2.303\times 5\times 8.314{\log }_{10}\frac{100}{10}=95.7J{K}^{-1}$
(because ‘S’ is a state function).
C) $\Delta S_{X\to Y}=95.7J{K}^{-1}$ (Reversible isothermal expansion)
D) Since ‘S’ is a state function, so  
 $$\begin{gathered} \Delta S_{X\to Y}=\Delta S_{X\to Z}+\Delta S_{Z\to Y}=95.7J{K}^{-1} \\ =0+\Delta S_{z\to y}=95.7 \end{gathered}$$
So, A,C and D correct