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 $K$)

One mole of an ideal diatomic gas $(C_V = 5 \ cal)$ was transformed from initial $25 \ ^{\circ}C$ and $1 \ L$ to the state when temperature is $100 \ ^{\circ}C$ and volume $10 \ L$. The entropy change of the process can be expressed as $(R = 2 \ cal / mol \cdot K)$ :-

For which of the following processes is $\Delta S$ negative?

Why does the entropy of a substance increase with an increase in temperature?

Mixing of non-reacting gases is generally accompanied by

Which of the following substances has the highest entropy?