Sergey Bylikin, Gary Horner and, Brian Murphy Solutions for Chapter: Energetics and Thermochemistry (AHL), Exercise 4: Quick questions

Calculate the Gibbs free energy change for the following reaction in $\mathrm{kJ} {\mathrm{mol}}^{-1}$. Values for $∆{\mathrm{G}}_{\mathrm{f}}^{⊝}$ are listed in the table.${\mathrm{SO}}_3\left(\mathrm{g}\right) + {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\to {\mathrm{H}}_2{\mathrm{SO}}_4 \left(\mathrm{l}\right)$

(Write the value correctly upto one decimal place)
 

Calculate the Gibbs free energy change for the following reaction in $\mathrm{kJ} {\mathrm{mol}}^{-1}$. Values for $∆{\mathrm{G}}_{\mathrm{f}}^{⊝}$ are listed in the table.$2{\mathrm{NH}}_4\mathrm{Cl}\left(\mathrm{s}\right) + \mathrm{CaO}\left(\mathrm{s}\right) \to {\mathrm{CaCl}}_2 \left(\mathrm{s}\right) + {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right) + 2{\mathrm{NH}}_3 \left(\mathrm{g}\right)$

(Write the value correctly up to one decimal place)

Calculate the Gibbs free energy change for the following reaction in $\mathrm{kJ} {\mathrm{mol}}^{-1}$. Values for $∆{\mathrm{G}}_{\mathrm{f}}^{⊝}$ are listed in the table.${\mathrm{C}}_2{\mathrm{H}}_4\left(\mathrm{g}\right) + {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\to {\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}\left(\mathrm{l}\right)$

(Write the value correctly upto two decimal places)