The entropy change involved in the isothermal reversible expansion of $2 \, \text{mole}$ of an ideal gas from a volume of $10 \, dm^3$ to a volume of $100 \, dm^3$ at $27 \, ^oC$ is : .............. $J \, K^{-1}$

Which of the following statements is incorrect when a system consisting of an ideal gas undergoes a change of state?

What is the entropy change (in $J\, K^{-1}\, mol^{-1}$) when one mole of ice is converted into water at $0^{\circ}C$? (The enthalpy change for the conversion of ice to liquid water is $6.0\, kJ\, mol^{-1}$ at $0^{\circ}C$)

At $1 \ atm$ pressure,if $\Delta S_{\text{vap}} = 75 \ J \ K^{-1} \ mol^{-1}$ and $\Delta H_{\text{vap}} = 30 \ kJ \ mol^{-1}$,what will be the boiling point of the liquid in $K$?

Match the following processes with their corresponding entropy changes:

$a$. Liquid to vapor conversion	$1$. $\Delta S = 0$
$b$. Reaction not spontaneous at any temperature,$\Delta H = (+)$	$2$. $\Delta S = (+)$
$c$. Reversible expansion of an ideal gas	$3$. $\Delta S = (-)$

Fill in the blanks:
$(i)$ The entropy of one mole of a substance at a fixed temperature and standard state is called ........ .
$(ii)$ The unit of molar entropy is .......... .
$(iii)$ The process of conversion of graphite into diamond is of ........ type.