The first step in industrial nitric acid production is the catalyzed oxidation of ammonia. Without a catalyst, a different reaction predominates:
4NH3(g) + 3O2(g) ⇔ 2N2(g) + 6H2O(g)
When 0.0180 mol gaseous NH3 and 0.0100 mol gaseous O2 are placed in a 1.00 L container at a certain temperature, the N2 concentration at equilibrium is 1.50×10-3 M.
Calculate Keq for the reaction at this temperature.

Question

The first step in industrial nitric acid production is the catalyzed oxidation of ammonia. Without a catalyst, a different reaction predominates: 
4NH3(g) + 3O2(g) ⇔ 2N2(g) + 6H2O(g) 
When 0.0180 mol gaseous NH3 and 0.0100 mol gaseous O2 are placed in a 1.00 L container at a certain temperature, the N2 concentration at equilibrium is 1.50×10-3 M. 
Calculate Keq for the reaction at this temperature.

anonymous · Answer

at eq mol N2 = 0.0015
         mol NH3 = 0.018 - 0.0015 = 0.00165
         mol O2 = 0.01 - 0.0015  = 0.0085
$$K _{eq} = \frac{ [N _{2}]^{2}[H _{2}O]^{6} }{ [NH _{3}]^{4}[O _{2}]^{3} }$$

anonymous · Answer

$$K _{eq} = \frac{ (0.0015)^{2}(0.0015) ^{6}}{ (0.0165)^{4}(0.0085)^{3} }$$
* mol of NH3 = 0.0165

anonymous · Answer

it says that is wrong..