A calorimeter contains 35.0 mL of water at 14.5 °C . When 1.30 g of X (a substance with a molar mass of 74.0 g/mol ) is added, it dissolves via the reaction X(s) H20(1)-*X(aq)
and the temperature of the solution increases to 25.0 ‘C
Calculate the enthalpy change, AH, 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. Express the change in enthalpy in kilojoules per mole to three significant figures.
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