If $900 \ J/g$ of heat is exchanged at the boiling point of water,what is the increase in entropy in $J \ K^{-1} \ mol^{-1}$?

In which of the following processes does the entropy decrease?

For a spontaneous process,the correct statement is

Considering entropy $(S)$ as a thermodynamic parameter,what are the necessary conditions for a process to be spontaneous?

$STATEMENT-1:$ There is a natural asymmetry between converting work to heat and converting heat to work.
$STATEMENT-2:$ No process is possible in which the sole result is the absorption of heat from a reservoir and its complete conversion into work.

The value of $\Delta S$ for freezing of $10 \ g$ of $H_2O_{(l)}$ (enthalpy of fusion is $80 \ cal/g$) at $0 \ ^\circ C$ and $1 \ atm$ pressure is.......$J/K$