Calculate the entropy change when $1 \, \text{mole}$ of ice is converted into water at $0 \, ^\circ\text{C}$. (The enthalpy change for the conversion of ice to liquid at $0 \, ^\circ\text{C}$ is $6.0 \, \text{kJ} \, \text{mol}^{-1}$).

Amongst the chemical reactions given below, the reactions with increasing entropy are
$(i)$ $H_2O_{(l)} \rightarrow H_2O_{(g)}$
$(ii)$ $C_{(s)} + CO_{2(g)} \rightarrow 2CO_{(g)}$
$(iii)$ $2H_{2(g)} + O_{2(g)} \rightarrow 2H_2O_{(l)}$
$(iv)$ $N_{2(g)} + O_{2(g)} \rightarrow \text{Mixture of } N_2 \text{ and } O_2$

In which of the following reactions is $\Delta S$ maximum?

What is the change in entropy of the surroundings for the reaction, $H_2(g) + 1/2 O_2(g) \rightarrow H_2O(l)$ at $298 \text{ K}$, if the standard enthalpy of formation of water is $-286 \text{ kJ mol}^{-1}$?

What is the entropy change in $J K^{-1}$ during the melting of $27.3 \ g$ of ice at $0^{\circ} C$? (Latent heat of fusion of ice $= 330 \ J g^{-1}$)

The entropy change in the isothermal reversible expansion of $2 \, \text{moles}$ of an ideal gas from $10 \, L$ to $100 \, L$ at $300 \, K$ is $..... \, J \, K^{-1}$.