Ialready posted this question, but im still confused on it.
dinitrogentetraoxide partially decomposes according to the following equilibrium:
n2o4 (g) -> 2no2 (g) < - a 1.00-l flask is charged with 0.400 mol of n2o4. at equilibrium at 373 k, 0.0055 mol ofn2o4
remains. keq for this reaction is ? . so my steps: n2o4 (g) -> 2no2 (g) initial conc. 0.400 mol 0 mole (no reaction yet) change -0.3945 mol + 2 x 0.3945 mole (based on equation above)
equilibrium 0.400-0.3945 mol 0.7890 mole 0.0055 mol 0.7890 keq = [no2]2/[n2o4] keq = (0.789)^2/(0.0055) =113 but my book says the answer is 0.87?