A calorimeter contains 31.0 mL of water at 15.0 ∘C . When 2.50 g of X...

A calorimeter contains 31.0 mL of water at 15.0 ∘C . When 2.50 g of X (a substance with a molar mass of 62.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 28.5 ∘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.

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queen_honey_blossom answered 1 year ago

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