Balance the chemical equation given below and calculate the

Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. ________ NH3(g) + ________ O2(g) ________ NO(g) + ________ H2O(l)

Solution

4 NH3 + 5 O2 4 NO + 6 H2O

(8.00 g NH3) / (17.03056 g NH3/mol) = 0.46974 mol NH3
(12.0 g O2) / (31.99886 g O2/mol) = 0.37501 mol O2

0.37501 mole of O2 would react completely with 0.37501 x (4/5) = 0.300008 mole of NH3, but there is more NH3 present than that, so NH3 is in excess and O2 is the limiting reactant.

(0.37501 mol O2) x (4 mol NO / 5 mol O2) x (30.00615 g NO/mol) / (1.23 g/L) = 7.32 L