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.
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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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5e3eb5b9-70f9-4c46-81e8-c844c47acf22%2F3c7ed562-e4f6-440f-94c2-5bc3da2ac55f%2F1be77l_processed.jpeg&w=3840&q=75)
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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