Posted by **tomi** on Wednesday, October 8, 2008 at 5:29pm.

A calorimeter contains 16.0ml of water at 15.0degrees celsius. When 1.60g of X(a substance with a molar mass of 46.0g/mol) is added, it dissolves via the reaction

X(s)+H20(l)->X(aq)

and the temperature of the solution increases to 25.0degrees celsius.

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

Assume that the specific heat and density of the resulting solution are equal to those of water [4.18j/g*C and 1.00g/ml] and that no heat is lost to the calorimeter itself, nor to the surroundings.

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