(a) Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide.CaCl₂(s)Cal₂(s)Lattice Energy-2247 kJ/mol-2059 kJ/mol*Explain.ΔΗsoln-46 kJ/mol-104 kJ/mol*Lattice energy is defined as the energy change for the process M*(g) + X¯(g) → MX(s).calcium chloride2201calcium iodide1955XkJ/molX kJ/mol(b) Based on your answers to part (a), which ion, CI or I, is more strongly attracted to water?chlorideiodideThe enthalpy of hydration for CaCl₂ is moreexothermic than for Cal2. Any differences must be due to differences in hydrations between CI and I¯.

Lattice energy is energy released when 1 equivalents of gaseous cation and gaseous anion react to…

(a) Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. Lattice Energy* -2247 kJ/mol -2059 kJ/mol CaCl₂(s) Cal₂(s) AH soln -46 kJ/mol -104 kJ/mol *Lattice energy is defined as the energy change for the process M*(g) + X¯(g) → MX(s). calcium chloride 2201 x kJ/mol calcium iodide 1955 X kJ/mol (b) Based on your answers to part (a), which ion, CI or I, is more strongly attracted to water? Ochloride O iodide Explain. The enthalpy of hydration for CaCl₂ is more exothermic than for Cal₂. Any differences must be due to differences in hydrations between CI and I.

(a) Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. Lattice Energy* -2247 kJ/mol -2059 kJ/mol CaCl₂(s) Cal₂(s) AH soln -46 kJ/mol -104 kJ/mol Lattice energy is defined as the energy change for the process M(g) + X¯(g) → MX(s). calcium chloride 2201 x kJ/mol calcium iodide 1955 X kJ/mol (b) Based on your answers to part (a), which ion, CI or I, is more strongly attracted to water? Ochloride O iodide Explain. The enthalpy of hydration for CaCl₂ is more exothermic than for Cal₂. Any differences must be due to differences in hydrations between CI and I.

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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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

(a) Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide.
CaCl₂(s)
Cal₂(s)
Lattice Energy
-2247 kJ/mol
-2059 kJ/mol
*
Explain.
ΔΗ
soln
-46 kJ/mol
-104 kJ/mol
*Lattice energy is defined as the energy change for the process M*(g) + X¯(g) → MX(s).
calcium chloride
2201
calcium iodide
1955
XkJ/mol
X kJ/mol
(b) Based on your answers to part (a), which ion, CI or I, is more strongly attracted to water?
chloride
iodide
The enthalpy of hydration for CaCl₂ is more
exothermic than for Cal2. Any differences must be due to differences in hydrations between CI and I¯.

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