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Br (aq) -121.6 (a) Calculate the enthalpy of dissolution for KBr(s) from the data. The lattice enthalpy of an ionic solid is the enthalpy of the reaction that forms the gas-phase ions from the solid, as represented in the chemical equation below. KBr(s) → K*(g) +Br(g) AH°, lattice =+691 kJ/mol,xn TX. (b) Calculate the enthalpy of the hydration reaction for KBr represented below: K*(g) + Br(g) → K*(aq) + Br (aq) AH° hydration=? (c) Identify the bonds broken in the lattice reaction and the bonds formed in the hydration reaction an give the relative values of these interactions based on the data for KBr.

Br (aq) -121.6 (a) Calculate the enthalpy of dissolution for KBr(s) from the data. The lattice enthalpy of an ionic solid is the enthalpy of the reaction that forms the gas-phase ions from the solid, as represented in the chemical equation below. KBr(s) → K*(g) +Br(g) AH°, lattice =+691 kJ/mol,xn TX. (b) Calculate the enthalpy of the hydration reaction for KBr represented below: K*(g) + Br(g) → K*(aq) + Br (aq) AH° hydration=? (c) Identify the bonds broken in the lattice reaction and the bonds formed in the hydration reaction an give the relative values of these interactions based on the data for KBr.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
Problem 79QRT
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238 CHAPTER 8 4. Consider the dissolution reaction of potassium bromide (KBr, M = 119,01 g/mol) represented by the chemical equation below: KBr(s) → K*(aq) + Br (aq) Thermodynamic data for solid and aqueous KBr are shown in the table below: AH formation (kJ/mol) Substance KBr(s) -393.8 K*(ag) -252.4 Br (aq) -121.6 (a) Calculate the enthalpy of dissolution for KBr(s) from the data. The lattice enthalpy of an ionic solid is the enthalpy of the reaction that forms the gas-phase ions from the solid, as represented in the chemical equation below. KBr(s) K*(g) + Br(g) AH° lattice = +691 kJ/mol. (b) Calculate the enthalpy of the hydration reaction for KBr represented below: K*(g) + Br (g) →K*(aq)+ Br (aq) ΔΗ. hydration = ? (c) Identify the bonds broken in the lattice reaction and the bonds formed in the hydration reaction an give the relative values of these interactions based on the data for KBr.
Transcribed Image Text:238 CHAPTER 8 4. Consider the dissolution reaction of potassium bromide (KBr, M = 119,01 g/mol) represented by the chemical equation below: KBr(s) → K*(aq) + Br (aq) Thermodynamic data for solid and aqueous KBr are shown in the table below: AH formation (kJ/mol) Substance KBr(s) -393.8 K*(ag) -252.4 Br (aq) -121.6 (a) Calculate the enthalpy of dissolution for KBr(s) from the data. The lattice enthalpy of an ionic solid is the enthalpy of the reaction that forms the gas-phase ions from the solid, as represented in the chemical equation below. KBr(s) K*(g) + Br(g) AH° lattice = +691 kJ/mol. (b) Calculate the enthalpy of the hydration reaction for KBr represented below: K*(g) + Br (g) →K*(aq)+ Br (aq) ΔΗ. hydration = ? (c) Identify the bonds broken in the lattice reaction and the bonds formed in the hydration reaction an give the relative values of these interactions based on the data for KBr.
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