The enthalpy of vaporization of benzene is $+35.3 \ kJ/mol$ at its boiling point,$80^{\circ} C$. The entropy change in the transition of vapour to liquid at its boiling point is

Calculate the entropy change in the surroundings when $1.00 \ mol$ of $H_2O_{(l)}$ is formed under standard conditions. Given: $\Delta_f H^{\theta} = -286 \ kJ \ mol^{-1}$.

For a reversible adiabatic expansion of an ideal gas,which of the following is equal to zero?

Given the standard entropy values at $298 \ K$ and $1 \ atm$ as $H_2(g) : 130.6 \ J \ K^{-1} \ mol^{-1}$,$Cl_2(g) : 223.0 \ J \ K^{-1} \ mol^{-1}$,and $HCl(g) : 186.7 \ J \ K^{-1} \ mol^{-1}$,calculate the entropy change $(\Delta S^{\circ})$ in $J \ K^{-1} \ mol^{-1}$ for the reaction: $H_2(g) + Cl_2(g) \rightarrow 2HCl(g)$

Identify the correct statement regarding a spontaneous process.

For the conversion $C$ (graphite) $\to C$ (diamond),the $\Delta S$ is: