Solid calcium carbonate (CaCO₃) decomposes into solid calcium oxide (CaO) and gaseous carbon dioxide (CO₂) in a constant-volume container at high temperatures. CO₂ is assumed to be an ideal gas, and the two solids are assumed to be in separate phases. You can vary the initial number of moles of CaCO₃, CaO, and CO₂ in the constant-volume container using sliders; the container displays the equilibrium pressure as the color intensity of the gas phase increases as the number of moles of CO₂ increases. The bar graph on the right shows the number of moles present at equilibrium. The equilibrium constant K_eq changes as the temperature changes using the slider. The equilibrium constant is equal to the CO₂ pressure (in bar) divided by the standard-state pressure of 1 bar. Note that adding more CaO when CaO is already in the container (or adding more CaCO₃ when CaCO₃ is already in the container) at equilibrium does not change equilibrium because increasing the number of moles of a pure solid does not change its fugacity.

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About:

This simulation was made at the University of Colorado Boulder, Department of Chemical and Biological Engineering.  Authors: Rachael L. Baumann, Garrison Vigil

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