A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities...
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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 14.5 kJ/mol separation of solvent 19.8 kJ/mol formation of solute-solvent interactions -85.7 kJ/mol solute Calculate the enthalpy of solution in kilojoules per mole of solute. Enter your answer numerically in kilojoules per mole of solute. v View Available Hint(s) Hint 1. How to approach the problem The enthalpy of the overall solution process is the sum of the component enthalpies as shown in the following equation: AĦsoln -ΔΗ ΔΗ + ΔΗ When using this equation, be aware of the signs on all enthalpy terms. ν ΑΣΦ ? ΔΗom kJ/mol 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 14.5 kJ/mol separation of solvent 19.8 kJ/mol formation of solute-solvent interactions -85.7 kJ/mol solute Calculate the enthalpy of solution in kilojoules per mole of solute. Enter your answer numerically in kilojoules per mole of solute. v View Available Hint(s) Hint 1. How to approach the problem The enthalpy of the overall solution process is the sum of the component enthalpies as shown in the following equation: AĦsoln -ΔΗ ΔΗ + ΔΗ When using this equation, be aware of the signs on all enthalpy terms. ν ΑΣΦ ? ΔΗom kJ/mol
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Enthalpy of separation of solute 145 kJmol Enthalpy ... View the full answer
Related Book For
Introduction to Chemical Engineering Thermodynamics
ISBN: 978-0071247085
7th edition
Authors: J. M. Smith, H. C. Van Ness, M. M. Abbott
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