While how much of each "reactant" and "product" a system ends up with depends on a number of factors (including, for example, how much energy is released when substances react or the temperature of the system), this model focuses on the concentrations of the reactants. Ultimately the system comes to a state of equilibrium with some of the "reactants" and some of the "products" present. When nitrogen dioxide (NO2) combines with carbon monoxide (CO), the resulting products - nitrogen monoxide (NO) and carbon dioxide (CO2) - are colorless, causing the system to lose some of its reddish color. While all substances in the reaction are gases, we could actually watch such a system reach equilibrium as nitrogen dioxide (NO2) is a visible reddish colored gas. The reverse reaction (where carbon dioxide and nitrogen monoxide react to form carbon monoxide and nitrogen dioxide) is also possible. This can also be written as a single, reversible reaction:Ī classic real-life example of such a reaction occurs when carbon monoxide reacts with nitrogen dioxide to produce carbon dioxide and nitrogen monoxide (or, nitric oxide). This model simulates two simple reactions of four molecules. In fact, in all chemical systems atomic-level processes continue but in a balance that yields no changes at the macroscopic level. This means that the system "looks" like nothing is happening. Equilibrium is the term we use to describe a system in which there are no macroscopic changes. This model shows how a simple chemical system comes to different equilibrium states depending on the concentrations of the initial reactants. You can also Try running it in NetLogo Web If you download the NetLogo application, this model is included. (back to the library) Chemical Equilibrium Sample Models/Chemistry & Physics/Chemical Reactions NetLogo Models Library: Chemical Equilibriumīeginners Interactive NetLogo Dictionary (BIND)
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |