$\Delta S_{surr}$ for an exothermic reaction is

In which of the following processes is the maximum increase in entropy observed?

State the limitation of the second law of thermodynamics.

What happens to the total entropy of the system and surroundings during a spontaneous irreversible process?

Identify the incorrect statements from the following:
$I. \quad \Delta S_{\text{system}} = (\Delta S_{\text{total}} + \Delta S_{\text{surr.}})$
$II. A_{(l)} \rightarrow A_{(s)}$: for this process entropy change decreases
$III.$ Entropy units are $J K^{-1} mol^{-1}$

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