A calorimeter contains 35.0 mL of water at 12.0 ∘C . When 2.30 g of X...
A calorimeter contains 35.0 mL of water at 12.0 ∘C . When 2.30 g of X (a substance with a molar mass of 70.0 g/mol ) is added, it dissolves via the reaction
X(s)+H2O(l)→X(aq)
and the temperature of the solution increases to 26.5 ∘C .
Calculate the enthalpy change, ΔH, 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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