A calorimeter contains 26.0mL of water at 14.0\, ^{\circ}C . When 2.30g of \rm X (a substance with a molar mass of 46.0g/mol ) is added, it dissolves via the reaction rm X{(s)}+H_2O{(l)} \rightarrow X{(aq)} and the temperature of the solution increases to 29.5\, ^{\circ}C .
Calculate the enthalpy change, Delta H, for this reaction per mole of \rm X.
Assume that the specific heat and density of the resulting solution are equal to those of water [4.18 \rm J/(g \cdot {^\circ C}) and 1.00 \rm g/mL] and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures