A steel reaction vessel at 25 oC initially contained pure NO2 at a concentration of 2.0 x 10-4 mol/L. Some of the NO2 reacted to form N2O4 as described by the following equilibrum equation: 2NO2(g) N2O4(g) At equilibrium, the concentration of N2O4 was found to be 6.01 x 10-6 mol/L. What is the concentration-based equilibrium constant (Kc) for this reaction at 25 oC?

Question

A steel reaction vessel at 25 oC initially contained pure NO2 at a concentration of 2.0 x 10-4 mol/L.  Some of the NO2 reacted to form N2O4 as described by the following equilibrum equation:

2NO2(g)   <---------->   N2O4(g)

At equilibrium, the concentration of N2O4 was found to be 6.01 x 10-6 mol/L.  What is the concentration-based equilibrium constant (Kc) for this reaction at 25 oC?

aaronq · Answer

Write an equilibrium expression, make an I.C.E. table. With this you can find $[NO_2]$ at eq. and solve for the constant.

anonymous · Answer

your so helpful thank you