In a calorimetric experiment, $5\mathrm{.}73$ g of lithium hydroxide, LiOH, was dissolved in water. The temperature of the calorimeter rose from $20\mathrm{.}57\backslash$deg C to $30\mathrm{.}88\backslash$deg C$.$ What is $\backslash$Delta H for the solution process?

LiOH$($s$)->$ Li$+($aq$)+$ OH$($aq$)$

The heat capacity of the calorimeter and its contents is $547$ J$/\backslash$deg C$.?=$kJ$/$mol