${\mathrm{H}}_2{\mathrm{O}}_2$ dissociates into  ${\mathrm{H}}_2\mathrm{O}\left(l\right)\text{ and }{\mathrm{O}}_2\left(g\right)$. All the ${\mathrm{H}}_2{\mathrm{O}}_2$ present in 1 L of 3.36 volume ${\mathrm{H}}_2{\mathrm{O}}_2$ is allowed to dissociate completely and all the released ${\mathrm{O}}_2$ is used for the combustion of 1.56 g of diborane  $\left({\mathrm{B}}_2{\mathrm{H}}_6\right)$. If heat of combustion of ${\mathrm{B}}_2{\mathrm{H}}_6$ is -1900 kJ/mol, then heat released by combustion of 1.56 g of diborane with ${\mathrm{O}}_2$ produced by above ${\mathrm{H}}_2{\mathrm{O}}_2$ solution is –P kJ. Find value of P/95 . Given 1 mole of a gas occupies 22.4 L at STP.