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Use the following data to estimate ∆E for the reaction: Ba ( s ) + Br 2 ( g ) → BaBr 2 ( s ) Δ E = ? Lattice energy −1985 kJ/mol First ionization energy of Ba 503 kJ/mol Second ionization energy of Ba 965 kJ/mol Electron affinity of Br −325 kJ/mol Bond energy of Br 2 193 kJ/mol Enthalpy of sublimation of Ba 178 kJ/mol

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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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Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 3, Problem 144CWP
Textbook Problem
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Use the following data to estimate ∆E for the reaction:

Ba ( s ) + Br 2 ( g ) BaBr 2 ( s ) Δ E = ?

Lattice energy −1985 kJ/mol
First ionization energy of Ba 503 kJ/mol
Second ionization energy of Ba 965 kJ/mol
Electron affinity of Br −325 kJ/mol
Bond energy of Br2 193 kJ/mol
Enthalpy of sublimation of Ba 178 kJ/mol

Interpretation Introduction

Interpretation: The energy change of the given reaction with the given data is to be calculated.

Concept Introduction: The energy change of the given reaction is calculated by born Haber cycle.

To determine: The energy change in the given reaction.

Explanation of Solution

Explanation

Given

The balanced chemical equation for the given reaction is,

Ba(s)+Br2(g)BaBr2(s)

The lattice energy of BaBr2 is 1985kJ/mol .

The first ionization energy of Ba is 503kJ/mol .

The second ionization energy of Ba is 965kJ/mol .

The electron affinity of Br is 325kJ/mol .

The bond energy of Br2 is 193kJ/mol .

The enthalpy of sublimation of Ba is 178kJ/mol .

The energy change of the reaction is calculated by born Haber cycle by using the formula,

ΔE=(ΔEsub(Ba)+D(Br2)+I1(Ba)+I2(Ba)+2×E(Br)ΔElattice)

Where,

  • ΔE is the energy change of the reaction.
  • ΔEsub(Ba) is the enthalpy of sublimation of Ba

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Chapter 3 Solutions

Chemistry: An Atoms First Approach
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