The $∆{\mathrm{H}}^0$ for the mutarotation of glucose in aqueous solution

$\alpha -D\text{-glucose }\left(aq\right)⟶\beta \text{ - }D\text{-glucose }\left(\alpha q\right)$

has been measured in a microcalorimeter and found to be $-1.16 \mathrm{KJ}. {\mathrm{mol}}^{-1}$. The enthalpies of solution of the two forms of glucose have been determined to be 

$\mathrm{\alpha }-\mathrm{D}-\text{ glucose }\left(\mathrm{s}\right)⟶\mathrm{\alpha }-\mathrm{D}-\text{ glucose }\left(\mathrm{aq}\right)$

$\mathrm{\Delta }{H}^{\circ }=10.72\mathrm{kJ}{\mathrm{mol}}^{-1}$

$\beta -D-\text{ glucose }\left(s\right)⟶\beta -D-\text{ glucose }\left(aq\right)$

$\mathrm{\Delta }{H}^{\circ }=4.68{\mathrm{kJmol}}^{-1}$

Calculate $∆{\mathrm{H}}^0$ (in kJ/mol) for the mutarotation of solid $\alpha$-D-glucose to solid $\beta$-D-glucose :