The entropy change in the isothermal reversible expansion of $2$ moles of an ideal gas from $10 \ L$ to $100 \ L$ at $300 \ K$ is: (in $JK^{-1}$)

The enthalpy change for the transition of liquid water to steam is $37.3 \ kJ \ mol^{-1}$ at $373 \ K$. Find $\Delta S$ in $J \ mol^{-1} \ K^{-1}$.

In which of the following processes does the entropy decrease?

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 enthalpy of vaporisation of a liquid is $30 \ kJ \ mol^{-1}$ and entropy of vaporisation is $75 \ J \ K^{-1} \ mol^{-1}$. Calculate the boiling point of the liquid at $1 \ atm$. (in $K$)

Calculate the increase in entropy (approximate) of $3 \ mol$ of hydrogen gas as it changes from $300 \ K$ at $0.1 \ atm$ to $1000 \ K$ at $1 \ atm$ $(C_p = 7 \ cal \ K^{-1} \ mol^{-1})$. $[\log \ 3.33 \approx 0.52, \ \ln \ x = 2.3 \ \log \ x]$ .......$cal \ K^{-1}$