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Related Concept Videos

Chemical Equilibria: Systematic Approach to Equilibrium Calculations01:21

Chemical Equilibria: Systematic Approach to Equilibrium Calculations

656
Equilibrium calculations for systems involving multiple equilibria are often complex. For example, to calculate the solubility of a sparingly soluble salt in an aqueous solution in the presence of a common ion, one must consider all the equilibria in this solution. Calculations for these systems can be complicated and tedious, so a systematic approach with a series of steps is often helpful. The process is detailed below.
The first step is to identify all the chemical reactions involved, The...
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Dynamic Equilibrium02:20

Dynamic Equilibrium

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A reversible chemical reaction represents a chemical process that proceeds in both forward (left to right) and reverse (right to left) directions. When the rates of the forward and reverse reactions are equal, the concentrations of the reactant and product species remain constant over time and the system is at equilibrium. A special double arrow is used to emphasize the reversible nature of the reaction. The relative concentrations of reactants and products in equilibrium systems vary greatly;...
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The Small x Assumption02:20

The Small x Assumption

46.0K
If a reaction has a small equilibrium constant, the equilibrium position favors the reactants. In such reactions, a negligible change in concentration may occur if the initial concentrations of reactants are high and the Kc value is small. In such circumstances, the equilibrium concentration is approximately equal to its initial concentration.  This estimation can be used to simplify the equilibrium calculations by assuming that some equilibrium concentrations are equal to the initial...
46.0K
Phase Diagram01:19

Phase Diagram

5.8K
The phase of a given substance depends on the pressure and temperature. Thus, plots of pressure versus temperature showing the phase in each region provide considerable insights into the thermal properties of substances. Such plots are known as phase diagrams. For instance, in the phase diagram for water (Figure 1), the solid curve boundaries between the phases indicate phase transitions (i.e., temperatures and pressures at which the phases coexist).
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Homogeneous Equilibria for Gaseous Reactions02:15

Homogeneous Equilibria for Gaseous Reactions

24.7K
Homogeneous Equilibria for Gaseous Reactions
For gas-phase reactions, the equilibrium constant may be expressed in terms of either the molar concentrations (Kc) or partial pressures (Kp) of the reactants and products. A relation between these two K values may be simply derived from the ideal gas equation and the definition of molarity. According to the ideal gas equation:
24.7K
Calculating Equilibrium Concentrations02:05

Calculating Equilibrium Concentrations

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Being able to calculate equilibrium concentrations is essential to many areas of science and technology—for example, in the formulation and dosing of pharmaceutical products. After a drug is ingested or injected, it is typically involved in several chemical equilibria that affect its ultimate concentration in the body system of interest. Knowledge of the quantitative aspects of these equilibria is required to compute a dosage amount that will solicit the desired therapeutic effect.
A more...
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Phase Behavior of Charged Vesicles Under Symmetric and Asymmetric Solution Conditions Monitored with Fluorescence Microscopy
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Efficient Approximation with Space Filling Quadtrees: Application to Phase Equilibria in Binary Mixtures.

Ian H Bell1

  • 1Applied Chemicals and Materials Division, National Institute of Standards and Technology, Boulder, Colorado 80305, United States.

Industrial & Engineering Chemistry Research
|October 9, 2024
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Summary
This summary is machine-generated.

This study introduces a novel method for creating fast and accurate numerical approximations of thermophysical properties. The technique ensures reliable convergence, outperforming traditional iterative methods in speed and efficiency for complex calculations.

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Area of Science:

  • Computational Chemistry
  • Chemical Engineering
  • Numerical Analysis

Background:

  • Thermophysical property calculations are crucial for chemical process design.
  • Existing iterative methods can be slow and prone to convergence failures, especially for mixtures.
  • Efficient function approximation is needed to overcome these limitations.

Purpose of the Study:

  • To develop a non-iterative numerical approximation technique for thermophysical properties.
  • To achieve high accuracy and computational efficiency in function representation.
  • To demonstrate the method's applicability to vapor-liquid equilibria calculations.

Main Methods:

  • Utilizing adaptive subdivision with quadtrees and bi-Chebyshev expansions.
  • Constructing a numerical approximation within a rectangular domain.
  • Employing bisection steps for rapid leaf identification in the approximation data structure.

Main Results:

  • The approximation function is evaluated in less than a microsecond.
  • Achieved accuracy is on the order of the noise in the original function.
  • For COSMO-SAC, the approximation is over 2000x faster with negligible deviations (<10⁻⁸).

Conclusions:

  • The proposed method offers a highly efficient and non-iterative approach for thermophysical property approximation.
  • This technique significantly accelerates calculations for models like COSMO-SAC.
  • The method provides a robust alternative to traditional iterative solvers, enhancing reliability and speed.