A reaction to convert ammonia into nitric acid involves following chemical
4 NH3 (g) + 5 O2 (g)à 4 NO(g) + 6 H2O(g)
Assume that 1.50 g of NH3 reacts with 2.75 g O2, then:
(a) Determine the limiting reactant.
(b) Calculate how many grams of NO and H2O will form in the reaction above.
Moles of Ammonia =
Moles of Oxygen
Mass of excess reactant that remain =
Moles of NO
Moles of H2O=
Limiting reactants is NH3
Where is the answer for (b) question?