Consider the following data: Lattice Energy CaCl2(s) –2247 kJ/mol –46 kJ/mol CaI2(s) –2059 kJ/mol –104 kJ/mol Calculate the enthalpy of hydration for calcium chloride. = kJ/mol Calculate the enthalpy of hydration for calcium iodide. = kJ/mol Based on your answers, which ion, Cl- or I-, is more strongly attracted to water?
Consider the following data: Lattice Energy CaCl2(s) –2247 kJ/mol –46 kJ/mol CaI2(s) –2059 kJ/mol –104 kJ/mol Calculate the enthalpy of hydration for calcium chloride. = kJ/mol Calculate the enthalpy of hydration for calcium iodide. = kJ/mol Based on your answers, which ion, Cl- or I-, is more strongly attracted to water?
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter10: Properties Of Solutions
Section: Chapter Questions
Problem 40E
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Consider the following data:
Lattice Energy | ||
CaCl2(s) | –2247 kJ/mol | –46 kJ/mol |
CaI2(s) | –2059 kJ/mol | –104 kJ/mol |
- Calculate the enthalpy of hydration for calcium chloride.
= kJ/mol
Calculate the enthalpy of hydration for calcium iodide.
= kJ/mol
- Based on your answers, which ion, Cl- or I-, is more strongly attracted to water?
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