The latent heat of melting of ice at $0^{\circ} C$ is $6 \, kJ \, mol^{-1}$. The entropy change during the melting in $J \, K^{-1} \, mol^{-1}$ is closest to

The standard entropies of $CO_{2(g)}$,$C_{(s)}$ and $O_{2(g)}$ are $213.5$,$5.690$ and $205 \ J \ K^{-1} \ mol^{-1}$ respectively. The standard entropy of formation of $CO_{2(g)}$ is ...... $J \ K^{-1} \ mol^{-1}$.

The enthalpy change for the transition of liquid water to steam at $373 \, K$ is $40.8 \, kJ \, mol^{-1}$. What is the $\Delta S$ for the process in $J \, K^{-1} \, mol^{-1}$?

For a spontaneous process,

Melting point of a solid is $x \ K$ and its latent heat of fusion is $600 \ cal \ mol^{-1}$. The entropy change for fusion of $1 \ mol$ solid is $2 \ cal \ mol^{-1} \ K^{-1}$. The value of $x$ will be......$K$

Predict in which of the following,entropy increases or decreases:
$(i)$ $A$ liquid crystallizes into a solid.
$(ii)$ Temperature of a crystalline solid is raised from $0 \, K$ to $115 \, K$.
$(iii)$ $2NaHCO_{3(s)} \to Na_2CO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$
$(iv)$ $H_{2(g)} \to 2H_{(g)}$