1. Consider the reaction of solid lead(II) oxide with ammonia gas to form elemental lead, gaseous molecular nitrogen and liquid water.

3PbO(s) + 2NH3(g) ---> 3Pb(s) + N2(g) + 3H2O(l)

Molar Mass: PbO = 223.20 g; NH3 = 17.04 g; Pb = 207.2

If you have 12.3 g of PbO and 33.6 g NH3 for the reaction,

(a) What will be the mass (g) of NH3 produced if the above-mentioned amount of PbO is consumed? (b) What mass (g) of PbO can be produced if the NH3 is fully consumed? (c) What will be the mass of the excess reactant left after completion of the reaction?