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Related Concept Videos

Calculating the Equilibrium Constant02:46

Calculating the Equilibrium Constant

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The equilibrium constant for a reaction is calculated from the equilibrium concentrations (or pressures) of its reactants and products. If these concentrations are known, the calculation simply involves their substitution into the Kc expression.
For example, gaseous nitrogen dioxide forms dinitrogen tetroxide according to this equation:
38.6K
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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Chemical Equilibria: Systematic Approach to Equilibrium Calculations01:21

Chemical Equilibria: Systematic Approach to Equilibrium Calculations

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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...
1.7K
The Nernst Equation02:59

The Nernst Equation

47.5K
Nonstandard Reaction Conditions
The interconnection between standard cell potentials and various thermodynamic parameters such as the standard free energy change ΔG° and equilibrium constant K has been previously explored. For example, a redox reaction involving zinc(II) and tin(II) ions at 1 M concentration with Eºcell = +0.291 V and ΔG° = −56.2 kJ is spontaneous.
47.5K
Dynamic Equilibrium02:20

Dynamic Equilibrium

63.8K
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;...
63.8K
Cell Potential and Free Energy02:58

Cell Potential and Free Energy

47.0K
Thermodynamics of a Redox Reaction
Thermodynamics is the branch of physics dealing with the relationship between heat and other forms of energy. In an electrochemical cell, chemical energy is converted into electrical energy.
Thus, a link can be predicted between cell potential, free energy change, and the equilibrium constant for the reaction. Cell potential can also be measured as the oxidant or the reducing strength, and similar acid-base strength measures are reflected in equilibrium...
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High-pressure Sapphire Cell for Phase Equilibria Measurements of CO2/Organic/Water Systems
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CFD analysis of laboratory scale phase equilibrium cell operation.

Mohamed Ali Jama1, Kaj Nikiforow1, Muhammad Saad Qureshi1

  • 1School of Chemical Technology, Department of Biotechnology and Chemical Technology, Research Group of Chemical Engineering, Aalto University, P.O. Box 16100, FI-00076 Aalto, Finland.

The Review of Scientific Instruments
|November 3, 2017
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Summary

Computational fluid dynamics (CFD) models gas-liquid equilibrium cells to ensure accurate chemical equilibrium data. This study validates CFD for predicting operating conditions where gas-liquid systems reach equilibrium, improving process modeling.

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Area of Science:

  • Chemical Engineering
  • Computational Science

Background:

  • Accurate chemical equilibrium data are crucial for modeling multiphase reactors and separation processes.
  • Traditional methods for verifying experimental equilibrium cells rely on assumptions that may not hold for all chemical systems due to mass transfer limitations.

Purpose of the Study:

  • To design and analyze a laboratory-scale experimental gas-liquid equilibrium cell using computational fluid dynamics (CFD).
  • To assess the validity of traditional analysis methods and determine operating conditions for achieving equilibrium in gas-liquid systems.

Main Methods:

  • Utilized CFD to model a two-phase dilutor cell for measuring limiting activity coefficients.
  • Employed a Lagrangian discrete model to track gas bubbles and analyze residence time distribution.
  • Calculated mass transfer for six bio-oil compounds to determine approach to equilibrium concentration.

Main Results:

  • CFD analysis provides a novel approach to designing and verifying gas-liquid equilibrium cells.
  • The study demonstrates that CFD can predict specific operating conditions where gas-liquid systems reach equilibrium.
  • Mass transfer calculations and residence time analysis highlight the influence of mixing on equilibrium attainment.

Conclusions:

  • CFD is a powerful tool for optimizing the design and operation of experimental equilibrium cells.
  • This approach enhances the reliability of chemical equilibrium data, essential for accurate process modeling.
  • The findings enable the prediction of optimal conditions for achieving equilibrium in diverse gas-liquid systems.