Gas-Phase Chemical Equilibrium at Constant Pressure or Constant Volume

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This Demonstration calculates the number of moles at equilibrium for a gas-phase reaction at constant temperature; the equilibrium constant for the reaction is . Components and are ideal gases, and you can set the value of (1/2, 1, 3/2, or 2) with buttons. Initially the container is filled with 5 mol of reactant , and equilibrium is obtained at either constant pressure (set pressure with a slider) or constant volume (set volume with a slider). The bar graph displays the number of moles at equilibrium, including the moles of inert gas (select the moles of inert with a slider). The height of the piston or container is proportional to the final volume.

Contributed by: Garrison J. Vigil and Rachael L. Baumann (July 2015)
Additional contributions by: John L. Falconer
(University of Colorado Boulder, Department of Chemical and Biological Engineering)
Open content licensed under CC BY-NC-SA


Snapshots


Details

The number of moles of each species in this reaction at equilibrium (values shown on the chart) determines the extent of reaction :

,

,

where and are the moles of reactant and product at equilibrium (mol), is the moles of reactant present initially, and is the ratio of moles of product to moles of reactant.

The equilibrium constant is:

,

where is the partial pressure of the reactant, is the partial pressure of the product, and is the total pressure (bar).

The mole fraction of each species at equilibrium is:

,

,

where the total number of moles is , with the number of moles of any inert component in the mixture.

The extent of reaction is found by setting and solving for .

The screencast video at [1] shows how to use this Demonstration.

Reference

[1] Gas-Phase Chemical Equilibrium at Constant Pressure or Constant Volume [Video]. (Sep 1, 2016) www.colorado.edu/learncheme/thermodynamics/Gas-PhaseChemicalEquilibriumatConstantPressureorConstantVolume.html.



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