Calculate the total entropy change for the transition at $368 \mathrm{K}$ of $1 \mathrm{mol}$ of sulphur from the monoclinic to the rhombic solid state and $\mathrm{\Delta H}=-401.7 \mathrm{J} {\mathrm{mol}}^{-1}$ for the transition. Assume the surroundings to be an ice-water bath at $0°\mathrm{C}:$

If $\mathrm{\Delta G}°=-177 \mathrm{K} \mathrm{cal}$ for $\left(1\right) 2{\mathrm{Fe}}_{\left(\mathrm{s}\right)}+\frac{3}{2}{{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}⟶{\mathrm{Fe}}_2{{\mathrm{O}}_3}_{\left(\mathrm{s}\right)}$

and $\mathrm{\Delta G}°=-19 \mathrm{K} \mathrm{cal}$ for $\left(2\right) 4{\mathrm{Fe}}_2{{\mathrm{O}}_3}_{\left(\mathrm{s}\right)}+{\mathrm{Fe}}_{\left(\mathrm{s}\right)}⟶3{\mathrm{Fe}}_3{{\mathrm{O}}_4}_{\left(\mathrm{s}\right)}$

What is the Gibbs free energy of formation of ${\mathrm{Fe}}_3{{\mathrm{O}}_4}_{\left(\mathrm{s}\right)}?$

Given the following data:

Determine at what temperature the following reaction is spontaneous?

$\mathrm{FeO}\left(\mathrm{s}\right)+\mathrm{C}\left(\mathrm{graphite}\right)\to \mathrm{Fe}\left(\mathrm{s}\right)+\mathrm{CO}\left(\mathrm{g}\right)$

The following curve represents the variation of Gibbs function '$\mathrm{G}$' with pressure at constant temperature.

Correct match of given plots with the physical state of a substance is