Why does the entropy of a substance increase with an increase in temperature?

Direct conversion of $A$ to $B$ is difficult,so it is carried out by the path shown below. If $e.u.$ is the entropy unit,what will be $\Delta S_{(A \rightarrow B)}$?
Given:
$\Delta S_{(A \rightarrow C)} = 50 \ e.u.$
$\Delta S_{(C \rightarrow D)} = 30 \ e.u.$
$\Delta S_{(B \rightarrow D)} = 20 \ e.u.$

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

The standard molar entropy of $H_{2}O_{(l)}$ is $70 \ J \ K^{-1} \ mol^{-1}$. Will the standard molar entropy of $H_{2}O_{(s)}$ be more or less than $70 \ J \ K^{-1} \ mol^{-1}$?

At $10\, ^oC$,$1\, mol$ of an ideal gas is allowed to expand reversibly and adiabatically from $10\, L$ to $200\, L$. Calculate the change in entropy in $cal/K$.

Standard entropy of $X_2, Y_2$ and $XY_3$ are $60, 40$ and $50 \ J \ K^{-1} \ mol^{-1},$ respectively. For the reaction,$\frac{1}{2}X_2 + \frac{3}{2}Y_2 \to XY_3, \ \Delta H = -30 \ kJ,$ to be at equilibrium,the temperature will be ............... $K$.