(Solved): Consider the following reaction at \( 298 \mathrm{~K} \). \[ 4 \mathrm{Al}(\mathrm{s})+3 \mathrm{O} ...

Consider the following reaction at \( 298 \mathrm{~K} \). \[ 4 \mathrm{Al}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(\mathrm{~s}) \quad \Delta H^{*}=-3351.4 \mathrm{~kJ} \] Calculate the following quantities. Refer to the standard entropy values as needed. Use the data from this table of thermodynamic properties to calculate the values of \( \Delta S_{\text {ixn }}^{*} \) for each of the reactions at \( 25^{\circ} \mathrm{C} \). \[ \mathrm{C}(\mathrm{s} \text {, graphite })+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \longrightarrow \mathrm{CO}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{~g}) \] \[ \Delta S_{\mathrm{fKn}}^{*} \] \[ \mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{~g}) \]