Textbook 5.39

[Kaleigh Olla 1L]

A problem in the textbook says:

In an experiment, 0.020 mol was introduced into a flask of volume 1.00 L and the reaction was allowed to come to equilibrium at 298 K. (a) Using information in Table 5G.2, calculate the equilibrium concentrations of the two gases. (b) The volume of the flask is reduced to half its original value. Calculate the new equilibrium concentrations of the gases

I set up my ice table, and set up K = x/((0.2-2x)^2) and solved for x. I keep getting the wrong answer, am I doing something wrong?

[Sharlene Duong 3E]

Hi! If you look on Dr. Lavelle's website he has a link to the solutions manual error. I believe the K value in the textbook is wrong for this problem. It should be 6.1x10^-3 instead of 6.1x10^23. You should also make sure that you do 1/K since you need the reverse reaction for this problem. Hope this helps!