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

What happens to the entropy during the melting of ice to water?

The enthalpy of vapourization of a liquid is $30 \ kJ \ mol^{-1}$ and entropy of vapourization is $75 \ J \ mol^{-1} \ K^{-1}$. The boiling point of the liquid at $1 \ atm$ is.......$K$

The entropy change when $2 \, \text{moles}$ of an ideal monoatomic gas is heated from $200 \, ^\circ \text{C}$ to $300 \, ^\circ \text{C}$ isochorically is:

Calculate $\Delta S_{\text{total}}$ for a certain reaction if $\Delta H = -150 \ kJ$ and $\Delta S = 32 \ JK^{-1}$ at $300 \ K$. (in $JK^{-1}$)

In which of the following processes does the entropy decrease?