When 2.89 g of AX (s) dissolves in 125.3 g of water in a coffee-cup calorimeter the temperature rises from 21.4 °C to 33.6 °C. Calculate the enthalpy change (in kJ/mol) for the solution process. AX (s) → A*(aq) + X¯ (aq) Assumptions for this calculation: • The specific heat of the solution is the same as that of pure water (4.18 J/gK) • The density of water = 1.000 g/mL • The liquid's final volume is not changed by adding the solid • The calorimeter loses only a negligible quantity of heat. The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change.

When 2.89 g of AX (s) dissolves in 125.3 g of water in a coffee-cup calorimeter the temperature rises from 21.4 °C to 33.6 °C. Calculate the enthalpy change (in kJ/mol) for the solution process. AX (s) → A*(aq) + X¯ (aq) Assumptions for this calculation: • The specific heat of the solution is the same as that of pure water (4.18 J/gK) • The density of water = 1.000 g/mL • The liquid's final volume is not changed by adding the solid • The calorimeter loses only a negligible quantity of heat. The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change.

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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