Problem- A calorimeter contains 17.0mL of water at 12.0?C . When 1.20g of X (a substance with a molar mass of 62.0g/mol ) is added, it dissolves via the reaction

X(s)+H2O(l)?X(aq)

and the temperature of the solution increases to 26.5?C .

Calculate the enthalpy change, ?H, for this reaction per mole of X.

Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g??C)], that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings

Please perform what you can and illustrate your work so I can follow. Thanks