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A calorimeter contains 29.0 mL of water at 13.0, ^{circ}C. When 2.40 g of rm X (a substance with a molar mass of 45.0 g/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 30.0, ^{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.

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Category:- Chemistry
Reference No.:- M9452419

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