1. 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.
(c) Calculate how many grams of the excess reactant will remain after the
reaction is complete.
(d) If the yield obtained for NO is 1.80 grams and yield obtained for H2O is 1.50
grams, calculate the percent yield of NO and H2O in this reaction.
(Atomic mass of N = 14 ; O = 16 ; H = 1)
a.) NH_3 is the limiting reagent.
c.) Moles of Ammonia = mol
Moles of Oxygen = = mol
Mass of excess reactant that remain = grams
Moles of NO moles
Moles of moles