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Calculating Standard Free Energy Changes02:49

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The free energy change for a reaction that occurs under the standard conditions of 1 bar pressure and at 298 K is called the standard free energy change. Since free energy is a state function, its value depends only on the conditions of the initial and final states of the system. A convenient and common approach to the calculation of free energy changes for physical and chemical reactions is by use of widely available compilations of standard state thermodynamic data. One method involves the...
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The free energy change associated with dissolving a solute in a liter of solvent is called the free energy of a solution, ΔGsolution. The overall ΔGsolution is expressed as the balance of ΔGinteraction against the always-favorable free-energy of mixing, ΔGmixing. Solution formation is favorable if  ΔGsolution is less than zero, whereas it is unfavorable if ΔGsolution is greater than zero. In short, for a solution to form and complete dissolution to take place,...
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The formation of a solution is an example of a spontaneous process, which is a process that occurs under specified conditions without energy from some external source.
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Solution, Solubility, and Solubility Equilibrium
A solution is a homogeneous mixture composed of a solvent, the major component, and a solute, the minor component. The physical state of a solution—solid, liquid, or gas—is typically the same as that of the solvent. Solute concentrations are often described with qualitative terms such as dilute (of relatively low concentration) and concentrated (of relatively high concentration).
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There are two criteria that favor, but do not guarantee, the spontaneous formation of a solution:
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The process of surrounding a solute with solvent is called solvation. It involves evenly distributing the solute within the solvent. The rule of thumb for determining a solvent for a given compound is that like dissolves like. A good solvent has molecular characteristics similar to those of the compound to be dissolved. For example, polar solutions dissolve polar solutes, and apolar solvents dissolve apolar solutes. A polar solvent is a solvent that has a high dielectric constant (ϵ...
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Calculating Free Energy Changes in Continuum Solvation Models.

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Direct free energy calculations using the SMD solvation model accurately predict solution phase kinetics and thermodynamics for diverse chemical reactions. This approach rivals traditional thermodynamic cycle calculations, offering reliable predictions for various systems.

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Area of Science:

  • Computational Chemistry
  • Physical Chemistry
  • Theoretical Chemistry

Background:

  • Continuum solvation models are crucial for calculating chemical properties in solution.
  • Previous work demonstrated the accuracy of direct free energy calculations within the SMD model for pKas and reduction potentials.

Purpose of the Study:

  • To evaluate the suitability of direct free energy calculations for general solution phase kinetics and thermodynamics.
  • To benchmark the performance of various solvation models, including SMD and CPCM, across a wide range of chemical systems.

Main Methods:

  • Utilized the SMD (Solvation Model based on Density) and CPCM (Conductor-like Polarizable Continuum Model) solvation models.
  • Calculated Gibbs free energy changes for neutral, radical, and ionic reactions, including enolization, atom transfer, and elimination/substitution reactions.
  • Employed cluster-continuum schemes for pKa calculations.

Main Results:

  • Direct SMD calculations show high accuracy, comparable to thermodynamic cycle calculations for various solvents.
  • Mean errors for Gibbs free energy changes were approximately 5 kJ/mol for neutral reactions and 25 kJ/mol for ionic reactions.
  • The direct approach demonstrated superior agreement with experimental data for systems with significant solvation-induced structural changes.

Conclusions:

  • Direct free energy calculations within continuum solvation models are reliable for predicting solution phase thermodynamics and kinetics.
  • The SMD model, particularly, offers a robust and accurate method for a broad spectrum of chemical reactions.
  • This approach is especially advantageous for systems exhibiting substantial changes in structure upon solvation.