Given: 

$\begin{array}{l}\text{ (1) }{\mathrm{HCO}}_3^{-}\left(\mathrm{aq}\right)+{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)\to {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)+{\mathrm{CO}}_3^{2-}\left(\mathrm{aq}\right):\hspace{0.25em} \hspace{0.25em}\hspace{0.25em}\hspace{0.25em} \mathrm{\Delta }{H}_1=-41.84\mathrm{kJ}{\mathrm{mol}}^{-1}\\ \text{ (2) }{\mathrm{H}}^{+}\left(\text{aq }\right)+{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)\to {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right):\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em} \mathrm{\Delta }{H}_2=-57.32\mathrm{kJ}{\mathrm{mol}}^{-1}\end{array}$

The enthalpy change for the reaction ${\mathrm{HCO}}_3^{-}\left(\mathrm{aq}\right)\to {\mathrm{H}}^{+}\left(\mathrm{aq}\right)+{\mathrm{CO}}_3^{2-}\left(\mathrm{aq}\right)$ would be