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?

Q: Expert Answer

(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. ΔH 0 = ∑ ΔH 0 f (product) − ∑ ΔH 0 f (reactant) Explanation By using Hess’s law the enthalpy change can be determined. CaCl 2(s) → Ca 2+ (g) +2Cl - (g) ΔH = -ΔH LE = - (-2247kJ) Ca 2+ (g) +2Cl - (g) → Ca 2+ (aq) +2Cl - (aq) ΔH = ΔH hyd CaCl 2(s) → Ca 2+ (aq) +2Cl - (aq) ΔH soln =-46kJ - 46kJ = 2247kJ + ΔH hyd ΔH hyd = -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. ΔH 0 = ∑ ΔH 0 f (product) − ∑ ΔH 0 f (reactant)

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

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Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Answer 3

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Answer 4

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Answer 5

(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

Answer 6

(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)

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

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The Solution to Your Study Problems

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Additional Science Textbook Solutions

	Lattice Energy	∆H_soln
CaCl₂(s)	−2247kj/mol	−46kj/mol
Cal₂(s)	−2059kj/mol	−104kj/mol

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach