For a spontaneous process,

Calculate the entropy change of the surrounding if $2 \ moles$ of $H_2$ and $1 \ mole$ of $O_2$ gas combine to form $2 \ moles$ of liquid water by releasing $525 \ kJ$ of heat to the surrounding at constant pressure and at $300 \ K$. (in $J \ K^{-1}$)

The standard entropies of $CO_{2(g)}$,$C_{(s)}$,and $O_{2(g)}$ are $213.5$,$5.740$,and $205 \ J \ K^{-1} \ mol^{-1}$ respectively. The standard entropy of formation of $CO_{2(g)}$ is $...... \ J \ K^{-1} \ mol^{-1}$.

Entropy is maximum in case of

The change of entropy $(dS)$ is defined as

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