A calorimeter contains 35.0 mL of water at 13.0 °C. When 1.80 g of X (a substance with a molar mass of 46.0 g/mol ) is added, it dissolves via the reaction X(s) + H2O(1)→X(aq) and the temperature of the solution increases to 25.0 °C. Calculate the enthalpy change, AH, 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.
A calorimeter contains 35.0 mL of water at 13.0 °C. When 1.80 g of X (a substance with a molar mass of 46.0 g/mol ) is added, it dissolves via the reaction X(s) + H2O(1)→X(aq) and the temperature of the solution increases to 25.0 °C. Calculate the enthalpy change, AH, 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.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 68E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...
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