Which of the following statements is true? The entropy of the universe

Standard entropies of $X_2, Y_2$ and $XY_5$ are $70, 50$ and $110 \ J \ K^{-1} \ mol^{-1}$ respectively. The temperature in Kelvin at which the reaction $\frac{1}{2} X_2 + \frac{5}{2} Y_2 \rightarrow XY_5$ with $\Delta H = -35 \ kJ \ mol^{-1}$ will be at equilibrium is . . . . . . (Nearest integer).

$3$ moles of water is boiled at $373 \ K$ and is changed to vapour state having the same temperature. What will be the change in entropy of the system (in $kJ/K$)? [ The molar heat of vaporization of water is $40.668 \ kJ/mol$ ]

Which of the following is the least $random$ state of water?

$18 \ g$ of ice is converted into water at $0 \ ^\circ C$ and $1 \ atm$. The entropies of $H_2O_{(s)}$ and $H_2O_{(l)}$ are $38.2$ and $60 \ J/mol \ K$ respectively. The enthalpy change for this conversion is ..... $J/mol$.

What is the change in entropy in $J \ K^{-1} \ mol^{-1}$ for the conversion of $1 \ mol$ of ice to water at $0 \, ^\circ C$? For the process $H_2O_{(s)} \rightarrow H_2O_{(l)}$ at $0 \, ^\circ C$,$\Delta H_{fus} = 6 \, kJ \ mol^{-1}$.