Consider the following reaction: 4nh3(g) 7o2(g) → 4no2(g) 6h2o(l) consider an experiment in which you react ammonia and oxygen. at the end of the experiment, you find that you produced 27.0 g of water, and 8.52 g of ammonia is left over. calculate the initial mass of ammonia. assume the reaction went to completion.

Initial mass of ammonia: 25,537g NH3

Explanation:

4NH3(g) 7O2(g) → 4NO2(g) 6H2O(l)

We have 4 Nitrogen atoms on both sides

12 Hydrogen atoms on both sides

14 Oxygen atoms on both sides

Final Mass of H2O = 27g  and Molecular Weigth = 18,015g/mol

Left Mass of NH3 = 8,52g and Molecular Weight= 17,031 g/mol

27g H2O  x  1mol H20/ 18,015 gH20  x 4mol NH3/ 6 mol H20 x 17,031g NH3 / 1mol NH3 = 17,017g NH3

17,017g NH3 were consumpted to generate 27 g of H2, however, lets remember that there is NH3 left, that must be added to finally discover the original amount

17,017g + 8,52g = 25,537g NH3

the answer is 0.42 is that is an option. this question provides no info