SOLVING EQUILIBRIUM PROBLEMS WITH THE TI-92
SOLVING EQUILIBRIUM PROBLEMS WITH THE TI-nspire
Chemical equilibrium is one of the most important topics you will study this year. An understanding of the basic principles of equilibrium will allow you to calculate the quantities of reactants and products at equilibrium for a wide variety of chemical systems. However, even simple systems, such as the Haber process to produce ammonia,
3 H2 (g) + N2 (g) [pic] 2 NH3 (g)
can require the solution of a cubic equation, and many reactions will require even higher orders. Fortunately, the
TI-nspire makes the exact mathematical solution of even these complicated equations quite simple. However, you must use your chemical knowledge to set up the appropriate equations, and interpret the results, if you are to obtain the correct answer. Remember the computer maxim, Garbage in, garbage out!
The key to correctly solving equilibrium problems is in setting up the ICE table, or reaction stoichiometry matrix. This will be covered in detail by your instructor, and the textbook; here, we are only interested in solving the equations that result. An example can be found in the following exercise, featuring an industrial process known as the water-gas shift reaction. What would be the equilibrium concentrations if 1.000 mol of each component were mixed in a 1.000 L container at 700 K, where the equilibrium constant has a value of 5.10? The reaction and ICE table for this system are shown below:
CO (g) + H2O (g) [pic] CO2 (g) + H2 (g)
Initial 1.000M 1.000M 1.000M 1.000M
Change -x -x +x +x ................
................
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