A calorimeter contains 17.0 of water at 12.5 degrees celsius . When 2.10 of (a s

Question

A calorimeter contains 17.0 of water at 12.5 degrees celsius . When 2.10 of (a substance with a molar mass of 80.0 g/mol) is added, it dissolves via the reaction and the temperature of the solution increases to 28.5 degrees . Calculate the enthalpy change, delta H, for this reaction per mole of . Assume that the specific heat and density of the resulting solution are equal to those of water [4.18 J/(g*degrees celesius) and 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.

Explanation / Answer

H = 4.18*(17*18gm+2.1*80gm)*(28.5-12.5) = 25.816 kJ/gm

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