   # a. Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. Lattice Energy ∆ H soln CaCl 2 ( s ) −2247kj/mol −46kj/mol Cal 2 ( s ) −2059kj/mol −104kj/mol b. Based on your answers to part a, which ion, Cl − or I − , is more strongly attracted to water? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 10, Problem 40E
Textbook Problem
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## a. Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide.   Lattice Energy ∆Hsoln CaCl2(s) −2247kj/mol −46kj/mol Cal2(s) −2059kj/mol −104kj/mol b. Based on your answers to part a, which ion, Cl− or I−, is more strongly attracted to water?

(a)

Interpretation Introduction

Interpretation:

Using given data enthalpy of hydration for Calcium chloride and Calcium Iodide to be calculated.

Concept introduction:

Hess’s law: Hess's law states that the change of enthalpy in a chemical reaction (i.e. the heat of reaction at constant pressure) is independent of the pathway between the initial and final states.

ΔH0=ΔH0f (product)ΔH0f (reactant)

### Explanation of Solution

By using Hess’s law the enthalpy change can be determined.

CaCl2(s)Ca2+(g)+2Cl-(g)ΔH = -ΔHLE= - (-2247kJ)Ca2+(g)+2Cl-(g)Ca2+(aq)+2Cl-(aq)ΔH = ΔHhydCaCl2(s)Ca2+(aq)+2Cl-(aq)ΔHsoln=-46kJ

- 46kJ = 2247kJ + ΔHhyd ΔHhyd= -2293kJ

CaI

(b)

Interpretation Introduction

Interpretation:

Based on part (a) answer, which ion Cl- or I- more strongly attracted to water has to be predicted.

Concept introduction:

Hess’s law: Hess's law states that the change of enthalpy in a chemical reaction (i.e. the heat of reaction at constant pressure) is independent of the pathway between the initial and final states.

ΔH0=ΔH0f (product)ΔH0f (reactant)

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