One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO:
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2
(a) Which is the limiting reactant?
(b) How many grams of NO and of H2O form?
(c) How many grams of the excess reactant remain after the limiting reactant is completely consumed?
(d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.