Compute the enthalpy change delta h

Reference no: EM13249827

A calorimeter contains 21.0 mL of water at 11.0\, ^{\circ}C. When 2.10 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 25.5\, ^{\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.

Reference no: EM13249827

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