A chemical engineer is studying the two reactions shown in the table below.

In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of $42\mathrm{.}0C$ and constant total pressure. Then, she measures the reaction enthalpy $H$ and reaction entropy $S$ of the first reaction, and the reaction enthalpy $H$ and reaction free energy $G$ of the second reaction. The results of her measurements are shown in the table.

Complete the table. That is$,$ calculate $G$ for the first reaction and $S$ for the second. $($Round your answer to zero decimal places.$)$ Then, decide whether, under the conditions the engineer has set up$,$ the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.

$\backslash$table$[[4Fe(s)+3O_2(g)2F{e}_2{O}_3(s),H=-1648,kJ$