A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 18.5 kJ/mol separation of solvent 19.8 kJ/mol formation of solute-solvent interactions -84.7 kJ/mol solute Calculate the enthalpy of solution in kilojoules per mole of solute.
A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 18.5 kJ/mol separation of solvent 19.8 kJ/mol formation of solute-solvent interactions -84.7 kJ/mol solute Calculate the enthalpy of solution in kilojoules per mole of solute.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![Part C
A solution is formed when the solute uniformly
disperses throughout (or dissolves in) the solvent.
The process can be described though three steps:
A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities
involved in the process are shown in the following table.
1. separation of solvent-solvent
particles,
2. breaking of solute-solute particles,
and
Action
Enthalpy
separation of solute
18.5 kJ/mol
3. formation of solute-solvent
interactions.
separation of solvent
19.8 kJ/mol
formation of solute-solvent interactions -84.7 kJ/mol solute
The overall energy change for the solution process,
AHsoln , is the sum of the enthalpies of the three
steps. Whether AHsoln is endothermic or
exothermic depends on the relative magnitudes of
AH1, AH2, and AH3, where the subscript
indicates the step in the process corresponding to
the enthalpy value.
Calculate the enthalpy of solution in kilojoules per mole of solute.
Enter your answer numerically in kilojoules per mole of solute.
• View Available Hint(s)
V ΑΣφ
?
AHsoln
– 50.4
kJ/mol
%3D
Submit
Previous Answers
X Incorrect; Try Again; 5 attempts remaining](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff89f5582-9fdc-4ede-82bb-28c01b8ca835%2F6c448530-182a-44b3-83e8-bdf7b1ce6349%2Frzu3vo_processed.png&w=3840&q=75)
Transcribed Image Text:Part C
A solution is formed when the solute uniformly
disperses throughout (or dissolves in) the solvent.
The process can be described though three steps:
A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities
involved in the process are shown in the following table.
1. separation of solvent-solvent
particles,
2. breaking of solute-solute particles,
and
Action
Enthalpy
separation of solute
18.5 kJ/mol
3. formation of solute-solvent
interactions.
separation of solvent
19.8 kJ/mol
formation of solute-solvent interactions -84.7 kJ/mol solute
The overall energy change for the solution process,
AHsoln , is the sum of the enthalpies of the three
steps. Whether AHsoln is endothermic or
exothermic depends on the relative magnitudes of
AH1, AH2, and AH3, where the subscript
indicates the step in the process corresponding to
the enthalpy value.
Calculate the enthalpy of solution in kilojoules per mole of solute.
Enter your answer numerically in kilojoules per mole of solute.
• View Available Hint(s)
V ΑΣφ
?
AHsoln
– 50.4
kJ/mol
%3D
Submit
Previous Answers
X Incorrect; Try Again; 5 attempts remaining
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