$2{\mathrm{H}}_{2\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}\to 2{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)};\mathrm{\Delta H}=-\text{ ve and }\mathrm{\Delta G}=-\mathrm{ve}$. Then the reaction is

$∆\mathrm{G}=-\mathrm{ve}$ indicates reaction is spontaneous

Bond rearrangement is more rate of reaction is less 

reaction is spontaneous and slow.