If the enthalpy of fusion of a compound at $27 \, ^\circ C$ is $2930 \, J/mol$,what is the entropy change in $J/mol \cdot K$?

For the reaction $2 H_{2(g)} + O_{2(g)} \longrightarrow 2 H_2O_{(g)}$,at $300 \ K$,$\Delta G$ and $\Delta H$ of water are $-228.4 \ kJ \ mol^{-1}$ and $-241.60 \ kJ \ mol^{-1}$,respectively. Calculate the value of change in entropy for the given reaction.

Which of the following is correct regarding entropy?

The spontaneous flow of heat is always

Statement-$1$: For a process at equilibrium,the total entropy is maximum and the change in total entropy is zero.
Statement-$2$: For a reversible process,if the same amount of heat is supplied to a system at two different temperatures,then the entropy change is less at a lower temperature.

The $\Delta S$ for the vaporisation of $1 \ mol$ of water is $88.3 \ J/mol \ K$. The value of $\Delta S$ for the condensation of $1 \ mol$ of vapour will be.......$ J/mol \ K$